U-2
UNIT-2 : SOLUTIONS
2007
1)State the condition resulting in reverse osmosis?
2) A 0.1539 molal aqueous solution of cane sugar (mol. Mass = 342 g mol-1) has a freezing point of 271 K
while the freezing point of pure water is 273.15 K. What will be the freezing point of a aqueous solution
containing 5 g of glucose ( mol mass = 180 g mol-1) per 100 g of solution?
1)State Raoult’s law for solutions of volatile liquid components. Taking a suitable example, explain positive
deviation from Raoult’s law.
2008
2)A solution containing 8g of a substance in 100g of diethyl ether boils at 36.86oc, whereas pure ether boils
at 35.60oc. Determine the molecular mass of the solute.( Foe ether, Kb= 2.02 K kg /mol.
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3) State the law co-relating the pressure of a gas and its solubility in a liquid. State an application of this
law.
4) Define the term ‘osmotic pressure’ . Describe how the molecular mass of a substance can be
determined on the basis of osmotic pressure measurement.
5) Calculate the temperature at which a solution containing 54 g glucose in 250 g water will freeze. (Kf for
water is 1.86 K Kg mol-1)
1)Define:
a) Mole fraction b) van’t Hoff factor
2)100mg of a protein is dissolved in enough water to make 10.0ml of a solution. If this solution has an
osmotic pressure of 13.3mm Hg at 25oc, what is the molar mass of the protein?( R=0.0821 L atm K-1mol-1
and 760mm Hg= 1 atm.)
3) What is meant by :
a) Colligative properties b) Molality of a solution
4. What conc of nitrogen should be present in a glass of water at room temp?
Assume a temp of 250C , a total pressure of 1 atmosphere and mol fraction of nitrogen in air of 0.78 ( KH for
nitrogen = 8.42 × 10-7 M / mm Hg)
1)Define osmosis and osmotic pressure? What is the advantage of using osmotic pressure over other
colligative properties.
2)What mass of NaCl (58.5 g/mol) must be dissolved in 65g water to lower the freezing point by 7.5oC?
Kf=1.86 K Kg/mol and I for Na Cl =1.86
3) Differentiate between molarity and molality of a solution.
4) 15 g of an unknown molecular substance was dissolved in 450 g of water. The resulting solution freezes
at -0.340C . What is the molar mass of the substance?
( Kf = 1.86 K Kg mol-1)
5) What mass of ethylene glycol ( molar mass = 62.0 g mol-1) must be added to 5.50 Kg of water to lower
the freezing point of water from 00C to -10.00C ? ( Kf = 1.86 K Kg mol-1)
1)State:
i)Raoult’s law in its general form in reference to solutions.
ii)Henry’s law about partial pressure of a gas in a mixture.
2)A solution is prepared by dissolving 8.95mg of a gene fragment in 35ml of water has an osmotic pressure
of 0.335 torr at 25oC. Calculate its molar mass if it is a non electrolyte.
3)What is reverse osmosis?
4)Difference between molarity and molality values for a solution. What is the effect of change in
temperature on molarity and molality values.
5) What mass of NaCl (58.5 g/mol) must be dissolved in 65g water to lower the freezing point by 7.5oC?
Kf=1.86 K Kg/mol and I for Na Cl =1.86
1) Define the following terms: (i) Mole fraction (ii) Ideal Solution
2) 15 g of an unknown molecular substance was dissolved in 450 g of water. The resulting solution freezes
at -0.340C . What is the molar mass of the substance? ( Kf = 1.86 K Kg mol-1)
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3) Explain the following :
(i) Henry’s Law about dissolution of gas in liquid
(ii) Boilling point elevation constant for a solvent
4) A solution of glycerol (C3H8O3) in water was prepared by dissolving some glycerol in 500 g of water. This
solution has a boiling point of 100.420C . What mass of glycerol was dissolved to make this solution? ( Kb
for water = 0.512 K Kg mol-1)
(a) State Raoult’s law for a solution containing volatile components. How does Raoult’s law become a special
case of Henry’s law ?
(b) 1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40
K. Find the molar mass of the solute. (Kf for benzene = 5.12 K kg mol–1)
(c ) Define the following terms :
(i) Ideal solution (ii) Azeotrope (iii) Osmotic pressure
(d) A solution of glucose (C6H12O6) in water is labelled as 10% by weight. What would be the molality of the
solution ? (Molar mass of glucose = 180 g mol–1)
1) a) Define the following terms: (i) Molarity (ii) Molal elevation constant (Kb)
b) A solution containing 15 g urea (molar mass= 60 g/mol) per litre of solution in water has the same osmotic
pressure (isotonic) as a solution of glucose (molar mass= 180 g/mol) in water. Calculate the mass of glucose
present in one litre of its solution.
Or
a) What type of deviation is shown by mixture of ethanol and acetone? Give reason.
b) A solution of glucose (molar mass = 180g/mol) in water is labelled as 10% (by mass). What would
be the molality and molarity of the solution?
(Density of solution + 1.2 g/mL) 2,3
(i) On mixing liquid X and liquid Y , the volume of the resulting solution increases. What type of deviation from
Raoult’s law is shown by the resulting solution? What change in temperature would you observe after mixing
liquids X and Y ?
(ii) How can the direction of osmosis be reversed ? Write one use of reverse osmosis.
(iii) A solution is prepared by dissolving 5 g of non volatile solute in 95 g of water. It has a vapour pressure of
23.375 mm Hg at 250C. Calculate the molar mass of the solute. ( Vapour pressure of pure water at 250C is 23.75
mm Hg)
(i) Write two differences between a solution showing positive deviation and a solution showing negative
deviation from Raoult’s law.
(ii) Calculate the freezing point of a solution when 3 g of CaCl2 ( M = 111 g mol-1) was dissolved in 100 g of
water, assuming CaCl2 undergoes complete ionization. ( Kf for water = 1.86 K kg mol-1)
(i) A 10% solution (by mass) of sucrose in water has a freezing point of 269.15 K. Calculate the freezing point of
10% glucose in water if the freezing point of pure water is 273.15 K. ( Molar mass of sucrose = 342 g mol-1,
Glucose = 180 g mol-1 )
(ii) Define a) Molality ( m) b) Abnormal molar mass
(iii) 30 g of urea ( M = 60 g mol-1 ) is dissolved in 846 g of water. Calculate the vapour pressure of water for this
solution if vapour pressure of pure water at 298 K is 23.8 mm Hg.
( iv) Write two differences between ideal and non ideal solutions.
(i)
Calculate the freezing point of a solution containing 60 g of glucose ( Molar Mass 180g/mol) in 250
g water (Kf for water = 1.86 K kg mol-1)
(ii)
Give reasons
a) Measurement of osmotic pressure method is preferred for the determination of molar masses of
macromolecules such as protein and polymers.
b) Aquatic animals are more comfortable in cold water than in warm water.
c) Elevation of b.pt of 1M KCl solution is nearly double than that of 1 M sugar solution.
Give reasons for the following : (a) Aquatic species are more comfortable in cold water than warm water.
(b) At higher altitudes people suffer from anoxia resulting in inability to think.
What type of azeotropic mixture will be formed by a solution of acetone and chloroform ? Justify on the
basis of strength of intermolecular interactions that develop in the solution.
At 300 K, 30 g of glucose present in a litre of its solution has an osmotic pressure of 4·98 bar. If the osmotic
pressure of a glucose solution is 1·52 bar at the same temperature, what would be its concentration ?
Unit-3
2007
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ELECTROCHEMISTRY
1)Define conductivity and molar conductivity for the solution of an electrolyte?
4+
2)On the v=basis of standard electrode potential values stated for acid solution, predict whether Ti species may be
II
III
used to oxidize Fe and Fe
O
Reaction
E /V
IV
3+
Ti + e - Ti
+0.01
3+
2+
Fe + e  Fe
+0.77
3 Calculate the standard cell potentials of galvanic cell in which the following reaction take place:
2+
3+
(i) 2Cr(s) + 3Cd (aq) → 2Cr (aq) + 3Cd
Calculate the ΔrG0 value for the reaction.
0
3+
0
2+
-1
Given E (Cr /Cr) = -0.74 V ; E ( Cd /Cd) = -0.40 V , F= 96500 C mol )
1)Express the relation between the conductivity and molar conductivity of a solution
2)Depict the galvanic cell in which the reaction
+
2+
Zn(s) + 2Ag (aq) Zn (aq) + 2Ag(s) Takes place. Further indicate what are the carriers of the current inside and
outside the cell. State the reactions at each electrode.
3)The resistance of a conductivity cell containing 0.001M KCl solution at 298K is 1500Ω. What is the cell constant if the
-3
-1
conductivity of 0.001M KCl solution at 298K is 0.146×10 S cm
–5
–1
4) Conductivity of 0.00241 M acetic acid is 7.896 × 10 S cm . Calculate its molar
0
2
–1
conductivity and if Λm for acetic acid is 390.5 S cm mol , what is its dissociation constant?
5) Three electrolytic cells A,B,C containing solutions of ZnSO4, AgNO3 and CuSO4,
respectively are connected in series. A steady current of 1.5 amperes was passed
through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of
copper and zinc were deposited?
1)What type of cell is a lead storage battery? Write the anode and cathode reactions and the overall cell reaction
occurring in the use of a lead storage battery?
2)A copper- silver cell is set up. The copper ion concentration in it is 0.10M. The concentration of silver ion in it is not
known The cell potential measured is 0.422V. Determine the concentration of silver ion in the cell.
O
O
(E Ag+/Ag=+0.80V, E Cu2+/Cu=0.34V
3) Two half cell reactions of an electrochemical cell are given below:
4+
2+
0
MnO + 8 H + 5e  Mn = 4H2O , E = + 1.51 V
2+
4+
0
Sn  Sn + 2e , E = + 0.15 VConstruct the redox equation and predict if this reaction favors the formation of
reactants or products shown in the equations.
0
4) A voltaic cell is set up at 25 C with the following half cells:
3+
2+
Al| Al (0.0010 M) and Ni | Ni (0.50 M)
Write the equation for the cell reaction that occurs when the cell generates an electric current and determine the cell
2+
3+
potential. (Given E0 (Ni /Ni) = -0.25 V , E0 (Al /Al) = -1.66 V)
1)Fluoride does not exhibit any positive oxidation state. Why?
2)Express the relation among the cell constant, the resistance of the solution in the cell and the conductivity of the
solution. How is the conductivity of a solution related to its molar conductivity?
O
3)Given that the standard electrode potentials (E ) of metals are
+
+
2+
2+
3+
2+
K +/K=-2.93v, Ag /Ag=0.80V,Cu /Cu=0.34V,Mg /Mg=2.97V,Cr /Cr=-0.74V, Fe /Fe=-0.44V.
Arrange these metals in an increasing order of their reducing power.
4) ) Two half cell reactions of an electrochemical cell are given below:
4+
2+
0
MnO + 8 H + 5e  Mn = 4H2O , E = + 1.51 V
2+
4+
0
Sn  Sn + 2e , E = + 0.15 V
Construct the redox equation and predict if this reaction favors the formation of
reactants or products shown in the equations.
1)a)What type of battery is a lead storage battery? Write the anode and cathode reactions and the overall cell
reaction occurring in the operation of a lead storage battery.
3+
-4
+
b)Calculate the potential for half cell containing 0.1M k2Cr2O7(aq), 0.2M Cr (aq) and 1.0 × 10 M H (aq). The half cell
+
3+
0
reaction is Cr2o7(aq)+14 H (aq)+ 6e 2Cr (aq) + 7H2o. ( Given E for half cell = 1.33 V)
1) Express the relation among cell constant, resistance of the solution in the cell and conductivity of the solution. How
is molar conductivity of a solution related to its conductivity?
2
-1
2) The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S cm mol . Calculate the
conductivity of this solution.
0
3) A voltaic cell is set up at 25 C with the following half cells:
3+
2+
Al| Al (0.0010 M) and Ni | Ni (0.50 M)
Write the equation for the cell reaction that occurs when the cell generates an electric current and determine the cell
2+
3+
potential. (Given E0 (Ni /Ni) = -0.25 V , E0 (Al /Al) = -1.66 V)
3
4) The electrical resistance of a column of 0.05 M NaOH solution of diameter 1 cm and length 50 cm is 5.55 × 10 ohm
. Calculate its resistivity , conductivity and molar conductivity.
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State Kohlrausch law. Why does the conductivity of a solution decrease with dilution?
o
2+
2+
o
(a) Calculate ΔrG for the reaction Mg (s) + Cu (aq)  Mg (aq) + Cu (s) Given: E cell = +2.71 V, 1F = 96500 C/mol
(b) Name the type of cell which was use in Apollo space programme for providing electrical power.
0
3) Define the fllowing terms:
2 i) Fuel Cell ii) Limiting molar conductivity (Ʌ m)
1. Calculate the time to deposit 1.17 g of ni at cathode when a current of 5 A was passed through the solution of
-1
-1
Ni(NO3)2. ( Molar mass of Ni=58.5 g mol , 1F = 96500 C mol )
0
0
2+
2+
2. Calculate E cell for the following reaction at 25 C : A + B ( 0.001 M )  A (0.0001 M) + B Given : Ecell = 2.6805 ,
1 F= 96500 C mol-1)
0
(a) Calculate ΔG and log Kc for the following reaction at 298 K:
2+
3+
0
2Al(s) + 3 Cu (aq)  2Al (aq) + 3 Cu (s)
Given : E cell = 2.02 V
0
0
2+
(b) Using the E values of A and B , predivt which is better for coating the surface of iron [ E ( Fe /Fe) = -0.14 V] to
0
2+
0
2+
prevent corrosion and why ? Given E ( A /A) = -2.37 V, E (B /B) = -0.14 V
-1
-5
-1
(c) The conductivity of 0.001 mol L solution of CH3COOH is 3.905 × 10 S cm . Calculate its molar conductivity and
0 +
2
-1
0
2
-1
degree of dissociation(α). Given λ (H ) = 349.6 S cm mol and
λ (CH3COO ) = 40.9 S cm mol
(d) What type of battery is dry cell ? Write the overall reaction occuring in dry cell.
1. Write the name of the cell used in hearing aids. Write the electrode reactions
2. Write the name of the cell used in inverters. Write the electrode reactions
3+
2+
3. The cell where the following reaction occurs 2Fe ( aq) + 2 I (aq)  2 Fe (aq) + I2 (s)
0
has E (cell) = 0.236 V at 298 K . Calculate the standard Gibbs energy of the cell reaction . ( Given : 1 F = 96500 C mol -1 )
-1
How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 h ? ( Given : 1 F = 96500 C mol )
a) Write the cell reaction and calculate the e.m.f. of the following cell at 298K:
b) Give reasons :
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(i) On the basis of E0 values, O2 gas should be liberated at anode but it is Cl2 gas which is liberated in
the electrolysis of aqueous NaCl. (ii) Conductivity of CH3COOH decreases on dilution.
c) (a) For the reaction, 2 AgCl (s) + H2 (g) (1 atm) ⎯⎯→ 2Ag (s) + 2H+ (0.1 M) + 2Cl– (0.1 M)
ΔGº = – 43600 J at 25ºC
Calculate the e.m.f. of the cell [log 10–n = –n]
(b) Define fuel cell and write its two advantages.
Explain with a graph, the variation of molar conductivity of a strong electrolyte with dilution.
U-4
Chemical Kinetics
2007
1. Express the rate of the following reaction in terms of disappearance of hydrogen in the reaction
3H2(g) + N2 (g)  2 NH3(g)
2. The rate constant for a first order reaction is 60 s-1 . How much time will it take to reduce the
concentration of the reactant ti 1/10 th of its initial value?
1. Derive the general expression for half life of a first order reaction.
2. The decomposition of NH3 on platinum surface is a zero order reaction . What would be the rates of
production of N2 and H2 if k = 2.5 × 10-4 mol L-1 s-1 ?
3. List the factors that determine the rate of a chemical reaction.
4. The half-life for radioactive decay of 14C is 5730 years. An archaeological artifact containing wood had
only 80% of the 14C found in a living tree. Estimate the age of the sample.
5. Define order of a chemical reaction.
6. A first order reaction takes 40 min for 30% decomposition. Calculate t1/2.
1. Define the following
(a) Elementary step in a reaction
(b) Rate of a reaction
2. A first order reaction has a rate constant of 0.0051 min-1 . If we begin with 0.10 M concentration of the
reactant , what conc of the reactant will be left after 3 hrs ?
3. For a decomposition reaction the values of rate constants k at two different temp. are given below:
k1 = 2.15 × 10-8 L mol-1 s-1 at 650 K
k1 = 2.39 × 10-7 L mol-1 s-1 at 700 K
Calculate the value of activation energy for this reaction. ( R= 8.314 J K-1 mol-1)
4. Define the following (a) Order of a reaction (b) Activation energy of a reaction
1. Define the following
(a) Activation energy of a reaction (b) Rate of a reaction
2. The decomposition of phosphine PH3 proceeds according to the following equation4PH3(g)  P4 (g) + 6H2(g)
It is found that the reaction follows the following rate equation : Rate = k[PH3]
The half life of PH3 is 37.9 sec at 120 0C
a) How much time is required for ¾ th of PH3 to decompose?
b) What fraction of the original sample of PH3 remains behind after 1 min ?
3. Explain a) Order of a reaction b) Molecularity of a reaction
4. The rate of a reaction increases 4 times when the temp changes from 300 K to 320 K . Calculate the
energy of activation of the reaction, assuming that it does not change with temp. ( R = 8.314 J K-1 mol-1)
1. Define order of a reaction.
2. What do you understand by rate law and rate constant of a reaction ? Identify the order of a reaction if
the units of its rate constants are
L-1 mol s-1
L mol-1 s-1
3. The thermal decomposition of HCOOH is a first order reaction with a rate constant of
2.4 × 10 -3 s-1 at a certain temp. Calculate how long will it take to form three-fourth of its initial quantity of
HCOOH to decompose ( log 0.25 = -0.6021 )
4. A reaction is second order w r t a reactant . How is the rate of reaction is affected if the concentration of
the reactant is reduced to half ? What is the unit of rate constant for such
a reaction ?
5. Define activation energy of a reaction.
1. A reaction is second order with respect to a reactant. How is the rate of reaction affected if the
concentration of the reactant is (i) doubled (ii) reduced to half ?
2. The reaction , N2 (g) + O2 (g) = 2 NO (g) contributes to air pollution whenever a fuel is burnt in air at a
high temp. At 1500 K , equilibrium constant K for it is 1.0 × 10-5 . Suppose in a case [N2] = 0.80 M and [O2] =
0.02 M before any reaction occurs. Calculate the equilibrium concentrations of the reactants and the
product after the mixture has been heated to 1500 K.
(a) For a reaction A + B → P, the rate law is given by r = k[A]1/2[B]2 What is the order of this reaction ?
(b) A first order reaction is found to have a rate constant k = 5.5 × 10–14 s–1. Find the half life of the reaction.
(c ) The rate of a reaction becomes four times when the temperature changes from 293 K to 313 K. Calculate the
energy of activation (Ea) of the reaction assuming that it does not change with temperature.
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[R = 8.314 J K–1 mole–1, log 4 = 0.6021]
2014
1) For chemical reaction R P yhe variation in the concentration (R) vs. time(t) plot is given as
Predict the order of the reaction. ii) What is the slope of the curve?
i)
2) The following data were obtained during the first order thermal decomposition of SO2Cl2 at const.
volume:
SO2Cl2 (g) SO2(g) +Cl2 (g)
Experiment
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Total pressure/atm
1
0
0.4
2
100
0.7
Calculate the rate const. (Given: log 4 =0.6021, log 2 = 0.3010)
1. For the hydrolysis of methyl acetate in aq soln, the following results were obtained:
t/s
[CH3COOCH3]/molL-1
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Times/s-1
0
0.04
20
0.02
40
0.01
a) Show that it follows pseudo first order reaction, as the conc of water remains constant.
b) Calculate the average rate of reaction between the time interval 20 to 40 s
2. Define the following terms : a) Collision frequency b) Rate constant (k)
3. The rate constant of a first order reaction increases from 4×10-2 to 24×10-2 when the temp changes from 300 K
to 350 K. Calculate the energy of activation (Ea)
(log2=0.301, log3=0.4771, log 4 = 0.6021 , log 6 = 0.7782)
1. Show that the time required for completion of 3/4th of the reaction of first order reaction is twice that of halflife of the reaction.
2. Derive integrated rate equation for rate constant of a zero order reaction.
3. For the first order thermal decomposition reaction , the following data were obtained
C2H5Cl (g)  C2H4(g) + HCl(g)
Time/sec
Total pressure/atm
0
0.30
300
0.50
Calculate the rate constant (Given : log 2 = 0.3010 log 3 = 0.4771 log 4 = 0.6021
1.What is the effect of adding a catalyst on Activation energy ( Ea) b) Gibbs energy ( ∆G) of a reaction
2.A first order reaction takes 20 minutes for 25% decomposition. Calculate the time when 75% of the
reactant will be completed. ( Given : log 2 = 0.3010, log 3 = 0.4771, log 4 = 0.6021
a) A first order reaction is 50 % completed in 40 minutes at 300 K and in 20 minutes at 320 K. Calculate the
activation energy of the reaction. (Given : log 2 = 0.3010, log 4 = 0.6021, R = 8.314 JK–1 mol–1)
b) For the reaction 2N2O5 (g) → 4NO2 (g) + O2 (g)
the rate of formation of NO2 (g) is 2.8 × 10–3 M s–1. Calculate the rate of disappearance of N2O5 g.
U-5
Surface Chemistry
2007
1. Describe the following types of colloids , giving an example for each:
a) Multimolecular colloids b) Macromolecular colloids
2. Explain with example: a) Shape selective catalysis b) Dialysis
1. Of physisorption and chemisorptions which type of adsorption has a higher enthalpy of adsorption?
2. Explain what is observed
(i) when a beam of light is passed through a colloidal sol.
(ii) an electrolyte, KCl is added to hydrated ferric oxide sol.
(iii) electric current is passed through a colloidal sol?
3. Differentiate between multimolecular and macromolecular colloids. Give one example of each. How are these
two types of colloids different from associated colloids?
4. Describe ‘electrophoresis’ briefly.
1. What is the ‘coagulation’ process? 2. Explain what is observed
(i) when a beam of light is passed through a colloidal sol. (ii) an electrolyte is added to hydrated ferric oxide
sol. (iii) an electric current is passed through a colloidal sol?
1. Describe the following :
a) Tyndall effect
b) Shape selective catalysis
2. What is meant by coagulation of a colloidal solution? Name any method by which coagulation of lyophobic
sols can be carried out.
3. Define the following: a) Peptization b) Reversible sols
1. What is meant by shape selective catalysis?
2. Classify colloids where the dispersion medium is water. State their characteristics and write an example of
each of these classes.
3. What are lyophobic colloids? Give one example for them.
1. Define peptization . 2. Explain the following terms with suitable example: a) Aerosol
b) Emulsion
c) Micelle 3. What is meant by shape selective catalysis?
4. Define peptization. 5. Write the distinct features of chemisorptions which are not found in physisorptions.
(a) Of physisorption or chemisorption, which has a higher enthalpy of adsorption ?
(b) Define the following terms given an example of each
(i) Associated colloids (ii) Lyophillic solution (iii) Adsorption
(c ) Give characteristics and example: (i) Multimolecular colloid (ii) Lyophobic sols (iii) Emulsions
1) What is the Effect of temperature on chemisorption?
2) What are emulsions? What are their different types? Give one example of each type.
3) Why is adsorption always exothermic?
1. What is the type of charge on AgI colloidal sol formed when AgNO3 solution is added to KI?
2. Differentiate between : a) solution and colloid b) homogeneous catalysis and heterogeneous catalysis
c) O/W emulsion and W/O emulsion
1. Write the main reason for the stability of colloidal sols
2. Define : a) Peptization b) Zeta potential b) Brownian movement
1. What type of colloid is formed when a liquid is dispersed in a solid ? Give an example.
2. What type of colloid is formed when a solid is dispersed in a liquid ? Give an example.
3. What type of colloid is formed when a gas is dispersed in a liquid ? Give an example.
4. Write one difference : a) Multimolecular and associated colloid
b) Coagulation and peptization c ) Homogeneuos and heterogeneous catalysis
5. Write the dispersed phase and dispersion medium of milk
6. Write one similarity between physisorption and chemisorptions
Write the chemical method by which Fe(OH)3 sol is prepared from FeCl3
i) CO (g) and H2 (g) react to give different products in the presence of different catalysts. Which ability of the
catalyst is shown by these reactions ?
ii) What happens when (a) a freshly prepared precipitate of Fe(OH)3 is shaken with a small amount of FeCl3
solution. (b) persistent dialysis of a colloidal solution is carried out ? (c) an emulsion is centrifuged ?
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Define associated colloid with an example.
Give reasons for the following : (a) Leather gets hardened after tanning. (b) FeCl3 is preferred over KCl in case
of a cut leading to bleeding. (c) Freundlich isotherm becomes independent of pressure at high pressure for a gas
absorbed on a solid.
Why are powdered substances more effective adsorbents than their crystalline forms ?
Write the main reason for the stability of colloidal sols.
Define the following terms with a suitable example of each : (a) Sol (b) Aerosol (c) Hydrosol
U-6
General Principles and Processes of Isolation of Elements
2008
a) What chemical principle is involved in choosing a reducing agent for getting the metal from its oxide ore?
Consider the metal oxides Al2O3 and Fe2O3 and justify the choice of reducing agent in each case.
a) What is meant by pyrometallurgy?
b) Describe the principle of:
(i) electrolytic refining of metal
(ii) vapour phase refining of metal
c) Describe the role of :
(i) NaCN in extraction of silver
(ii) Cryolite in extraction of aluminium.
a) Describe the role of :
(i) NaCN in extraction of silver
(ii) Cryolite in extraction of aluminium.
(iii) Iodine in refining of titanium.
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b) Describe the principle of:
(i) electrolytic refining of metal
(ii) froth floatation method
(iii) zone refining of metals
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2013
2014
a) Differentiate between a mineral and an ore.
b) Describe the principle of:
(i) vapour phase refining of titanium
(ii) froth floatation method for sulphide ores
(c ) Why is that sulphide ores are concentrated by froth floatation method
(d) Describe the principle of:
(i) electrolytic refining of metal
(ii) zone refining of metals
(e) What type of ores can be concentrated by magnetic separation method?
(a) How is copper extracted from a low grade ore of it?
(b) Which methods are usually employed to purify : (i) Ni (ii) Ge Mention the principle behind each of
them
(c) What is the role of collectors in froth floatation method?
(d) Describe the role of :
(i) NaCN in extraction of silver
(ii) SiO2 in extraction of copper.
(a) Outline the principles of refining of metals by the folliowing methods
(i) Zone refining (ii) Vapour phase refining
(b) Name the method used for refining of copper metal.
(C ) Name the method used for removing gangue from sulphide ore.
(d) How is wroght iron different from steel?
1) What is the role of zinc metal in the extraction of silver?
2) Explain the principle of the method of electrolytic refining of metals.Give one example.
3) Name the method that is used for refining of nickel.
4) Describe the role of the following:
(i)
SiO2 in the extraction of copper from copper matte (ii) NaCN in forth floatation process
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U-7
2007
2008
2009
1. Name the method of refining to obtain low boiling metal like mercury
2. What is the role of pine oil in froth floatation process?
3. Reduction of metal oxide to metal becomes easier if the metal obtained is in liquid state. Why ?
Write the principle of
a) Vapour phase refining b) Chromatography c) Froth floatation process
1. Write the principle of a) Zone refining b) Froth floatation process c) Chromatography
Write the chemical reactions involved in the process of extraction of Gold. Explain the role of dilute NaCN
and Zn in this process.
What is the role of (a) Depressants in froth floatation ? (b) Carbon monoxide in Mond’s process ? (c)
Concentrated sodium hydroxide in leaching of alumina from bauxite ?
Write chemical reactions taking place in the extraction of Aluminium from Bauxite ore.
The p-block Elements
Explain why
1. SF6 is less reactive than SF4
2. Of the noble gases only xenon forms compounds
3. In solid state PCl5 behaves as ionic compounds
4. Acidic strength increases : HF < HCl < HBr < HI
5. H3PO2 is mono protic acid
Draw the structures: SF4 , XeF2
Explain why
1. PH3 has lesser bond angle than NH3
2. Bi(V) is stronger oxidizing agent than Sb(V)
3. Sulphur vapour is paramagnetic
4. NH3 has greater affinity for proton than PH3
5. Negative value of electron gain enthalpy of F is less than that of Cl
6. SF6 is less reactive than SF4
7. Of the noble gases only xenon forms compounds
8. Acidic strength increases : HF < HCl < HBr < HI
9. Phosphorous shows catenation but nitrogen not
10. Negative value of electron gain enthalpy of O is less than that of S
11. P4 is more reactive than N2
12. All bonds in PCl5 are not equal in length
Draw the structures: PCl5(g) , S8 (g) , ClF3(g), H2S2O7 , NO3- , BrF3 , XeF2
Complete the reactions:
(i) F2 + H2O  (ii) Ca3P2 + H2O  (iii) XeF4 + H2O 
1. Which neutral molecule is isoelectronic with ClO- ?
2. Describe the favourable condition for manufacture of NH3 by Haber’s process and H2SO4 by contact process
Explain why
1. Red phosphorous is less reactive than white phosphorous
2. NH3 is stronger base than PH3
3. S has greater tendency for catenation than O
4. F2 is stronger oxidizing agent than Cl2
5. In HNO3 N-O bond is shorter than N-OH bond
6. All bonds in PCl5 are not equal in length
7. ICl is more reactive than I2
8. Phosphorous shows catenation but nitrogen not
9. Bond dissociation enthalpy of F2 is less than Cl2
10. No chemical compound of He is known
11. Negative value of electron gain enthalpy of O is less than that of S
12. N does not form penta halide
13. Acidic strength increases : HF < HCl < HBr < HI
14. Negative value of electron gain enthalpy of F is less than that of Cl
15. HF has higher bpt than HCl
16. NH3 has higher bpt than PH3
17. Bi(V) is stronger oxidizing agent than Sb(V)
Draw the structures: H2S2O8 , HClO4 , H2S2O7 , HClO3 , H3PO2 , BrF3 , N2O5, XeOF4, XeF4 , PCl5(s) , SO32-
Complete the reactions:
(i) XeF2 + H2O  (ii) PH3 + HgCl2 
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2014
Explain why
1. NCl3 is an endothermic compound while NF3 is an exothermic one
2. XeF2 is a linear compound without a bend
3. Negative value of electron gain enthalpy of F is less than that of Cl still fluorine is stronger oxidizing
agent than chlorine
4. Negative value of electron gain enthalpy of O is less than that of S
5. Phosphorous shows catenation but nitrogen not
6. F never acts as the central atom in polyatomic inter halogen compounds
7. Nitrogen is relatively inert than phosphorous
Draw the structures: H4P2O7 , XeF4
Complete the reactions:
(i) I2 + HNO3(conc) 
(ii) HgCl2 + PH3  (iii) NaOH (cold,dil) + Cl2  (iii) XeF6 + H2O 
Explain why
1. H2S is more acidic than H2O
2. The N-O bond in NO2- is shorter than that in NO33. The ability of oxygen to stabilize high oxidation states exceeds that of fluorine
4. H3PO3 is dibasic
5. F never acts as the central atom in polyatomic inter halogen compounds
6. Noble gases have very low bpt
7. NCl3 is an endothermic compound while NF3 is an exothermic one
8. Acidic strength increases : PH3 < H2S < HCl
Draw the structures: (HPO3)3 , BrF3 ,
Complete the reactions:
(i) HgCl2 + PH3  (ii) SO3 + H2SO4  (iii) XeF4 + H2O  (iv) Cl2 + NaOH(hot, conc) 
(v) SO2 + Fe3+ (aq) 
Explain why
1. SbH3 or BiH3 which one is stronger reducing agent and why?
2. NCl3 is an endothermic compound while NF3 is an exothermic one
3. All the bonds in SF4 are not equal
4. S has greater tendency for catenation than O
5. ICl is more reactive than I2
6. Negative value of electron gain enthalpy of F is less than that of Cl still fluorine(F2) is stronger oxidizing
agent than chlorine(Cl2)
7. Phosphorous shows catenation but nitrogen not
8. Oxygen is a gas but sulphur is a solid
9. The halogens are coloured
10. Nitrogen is relatively inert than phosphorous
11. Despite having greater polarity , HF boils at a lower temp than water
12. S has greater tendency for catenation than O
13. H2S is more acidic than H2O
14. Fluorine does not exhibit any positive oxidation state
15. No chemical compound of He is known
Draw the structures: N2O5 , XeOF4 , H3PO2 , ClF3 , HClO4
Complete the reactions: (i) Cu + HNO3(dil) 
(ii) XeF4 + O2F2 
Given reasons for the following :
(i) Oxygen is a gas but sulphur is a solid (ii) O3 acts as a powerful oxidizing agent
(iii) BiH3 is the strongest reducing agent amongst all the hydrides of group 15 elements
Draw the structures of the following molecules
(i) XeF6 (ii) H2S2O7
How are interhalogen compounds formed ? What general compositions can be assighed to them ?
Which aerosol depletes ozone layer ?
Draw : XeOF4, H3PO3
Explain:
(i)
R3P=O exists but R3N=O does not
(ii)
PbCl4 is more covalent than PbCl2
(iii)
At room temp . N2 is much less rreactive.
1) What is the basicity of H3PO3?
1
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2) Complete the following reaction2
(i)
P4 + H2O 
(ii) XeF4 + O2F2
3) Draw the structure of the following:
2
(i)
XeF2
(ii) BrF3
4) Give reason for the following:
3
(i)
(CH3)3P =O exist but (CH3)3N =O does not exist.
(ii)
Oxygen has the less electron gain enthalpy with negative sign than sulphur.
(iii)
H3PO2 is a stronger reducing agent than H3PO3.
5) Why does NO2dimerise?
1
6) Complete the following reaction
2
(i)
Ag + PCl5
(ii) CaF2 +H2SO4 
7) Draw the structure of the following: (i) XeF4
(ii) HClO4
1. Write the formula of any two oxoacids of chlorine
2. Explain why
a) Bi(V) is a stronger oxidizing agent than Sb(V) b) H-O-I is a weaker acid than H-O-Cl
c) Bond angle decreases from H2O to H2S
3. Draw the structures of the following : a) SF4 b) XeF2
4.Why does PCl5 fume in moisture?
5. Write the name of the allotrope of sulphur which is stable at room temp
6. Chlorine water on standing loses its yellow colour. Why?
7. Write the disproportionation reaction of H3PO3 8. Complete the following equation : F2 + H2O 
1. On heating Copper turnings with conc. H2SO4 , a colorless gas with pungent smell is evolved which decolourises
acidified KMnO4 solution. Identify the gas.
2. Write the structure : i) H2S2O8
ii) XeF6
3.Give reasons :
a) Red phosphorous is less reactive than white phosphorous b) S has greater tendency for catenation than O
c) ClF3 is known but FCl3 is not known
1.
2.
3.
4.
5.
Write the formula of the compound of phosphorous formed when conc HNO3 oxidizes P4
Write the formula of the compound of sulphur formed when conc HNO3 oxidizes S8
Write the formula of the compound of iodine formed when conc HNO3 oxidizes I2 ?
Draw the structure of : H2SO3 , HClO3 , H2S2O8 , ClF3 , XeF4 , BrF5
Give reasons :
a) Red phosphorous is less reactive than white phosphorous
b) Electron gain enthalpies of halogens are largely negative
c) N2O5 is more acidic than N2O3
1. Among the hydrides of Group-15 elements, which have the
(a) lowest boiling point ? (b) maximum basic character ? (c) highest bond angle ?
(d) maximum reducing character ?
2. (a) Give reasons :
(i) H3PO3 undergoes disproportionation reaction but H3PO4 does not.
(ii) When Cl2 reacts with excess of F2, ClF3 is formed and not FCl3.
(iii) Dioxygen is a gas while sulphur is a solid at room temperature.
(b) Draw the structures of the following (i) XeF4 (ii) HClO3
3. When concentrated sulphuric acid was added to an unknown salt present in a test tube a brown gas
(A)
was evolved. This gas intensified when copper turnings were added to this test tube. On cooling, the gas
(A) changed into a colourless solid (B)
(i) Identify (A) and (B)
(ii) Write the structures of (A) and (B) (iii) When does gas (A) change to
solid on cooling ?
(b) Arrange the following in the decreasing order of their reducing character
HF, HCl, HBr, HI
(c) Complete the following reaction :
XeF4 + SbF5 ⎯⎯→
When dilute ferrous sulphate solution is added to an aqueous solution containing nitrate ion followed by
careful addition of concentrated sulphuric acid along the sides of test tube, a brown ring is formed at the
interface between the solution and sulphuric acid layers. Which anion is confirmed by the appearance of
brown ring ? What is the composition of the brown ring ?
How can you prepare Cl2 from HCl and HCl from Cl2 ? Write reactions only.
(a) Draw the structure of the following : (i) HClO3 (ii) H2S2O8 (b) Give reasons for the following : (i)
Above 1000 K sulphur shows paramagnetism. (ii) Although electron gain enthalpy of fluorine is less
negative than that of chlorine, yet flourine is a better oxidising agent than chlorine. (iii) In solid state
PCl5 exists as an ionic compound.
U-8
2007
2008
2009
2010
2011
The d&f-block Elements
Explain why
1. Transition elements have higher enthalpy of atomization
2. Transition metals and their compounds act as good catalyst
Explain why
1. The transition metals generally form coloured compounds
2. With 3d4 configuration , Cr2+ acts as a reducing agent but Mn3+ acts as an oxidizing agent
3. The actinoids exhibit a larger number of oxidation states than the lanthanoids.
Complete the chemical equations
1. Oxidation of Fe2+ by Cr2O72- in acidic medium
2. Oxidation of S2O32- by MnO4- in neutral aqueous medium
Explain why
1. Transition metals and their compounds act as good catalyst
2. The metallic radii of the third (5d) series of transition elements are virtually the same as the
corresponding member of the second series.
3. The actinoids exhibit a larger number of oxidation states than the lanthanoids.
Complete the chemical equations
1. MnO4-(aq) + C2O42-(aq) + H+ (aq) 
2. Cr2O72- + Fe2+ + H+ 
Explain why
1. The oxidizing power of oxoanions are in the order VO2+ < Cr2O72- < MnO42. The third IE of Mn(Z=25) is exceptionally high
3. Cr2+ is a stronger reducing agent than Fe2+
4. La3+ (Z=57) and Lu3+ (Z=71) do not show any colour in aqueous soln.
5. Among divalent cation of 1st series transition elements Mn exhibits maximum paramagnetism.
6. Cu+ ion is not known in aqueous solutions
Complete the chemical equations
1. Cr2O72- + H2S(g) + H+(aq) 
2. Cu2+ (aq) + I- (aq) 
3. Oxidation of S2O32- by MnO4- in neutral aqueous medium
4. Cr2O72- + Fe2+ + H+ 
1. What is meant by ‘lanthanoid contraction’ ?
Explain why
1. With 3d4 configuration , Cr2+ acts as a reducing agent but Mn3+ acts as an oxidizing agent
2. In a transition series the metal which exhibits greatest number of oxidation states occurs in the
middle of the series
3. Cu+ ion is not known in aqueous solutions
4. Unlike Cr3+, Mn2+, Fe3+ of 3d series , the metals of 4d and 5d series generally do not form
any stable cation.
5. Transition metals and their compounds act as good catalyst
6. Metal-metal bonding is more frequent in 4d and 5d series than that of 3d series.
7. Transition metals and their compounds generally exhibit paramagnetic behavior
8. The chemistry of actinoids is not so smooth as that of lanthanoids
Complete the chemical equations
1. MnO4- (aq) + S2O32- (aq) + H2O(l) 
2. Cr2O72- + Fe2+ + H+ 
2012
Explain why
1. Among lanthanoids Ln(III) compounds are predominant. However , occasionally in solutions
or in solid compounds, +2 and +4 ions are also obtained.
2. The E0M2+/M for copper is positive (+0.34V). Copper is the only metal in first row of
transition series showing this behavior.
3. The metallic radii of the third (5d) series of transition elements are virtually the same as the
corresponding member of the second series.
4. Many transition metals are known to form interstitial compounds
5. Density increases from Ti to Cu
6. The actinoids exhibit a larger number of oxidation states than the lanthanoids.
7. With 3d4 configuration , Cr2+ acts as a reducing agent but Mn3+ acts as an oxidizing agent
8. There is hardly any increase in atomic size with increasing atomic number in a series of
transition metals
Complete the chemical equations
1. Cr2O72- + I- + H+ 
2. MnO4- + NO2- + H+ 
2013
(a) Given reasons for the following :
(i) Mn3+ is a good oxidizing agent
(ii) oEM2+ /M values are not regular for first row transition metals (3d series)
(iii) Although 'F' is more electronegative than 'O', the highest Mn fluoride is MnF4, whereas the
highestoxide is Mn2O7
(b) Complete the following equation :
(a) Why do transition elements show variable oxidation states ?
(i) name the elements showing maximum number of oxidation states among the first series of transtition
metals from Sc (Z = 21) to Zn (Z=30)
(ii) Name the element which shows only +3 oxidation state
(b) What is lanthanide contraction ? Name an important alloy which contains some of the lanthanoid metals
2014
1) a) Complete the following equations:
(i)
Cr2O72- +2OH-
(ii)
MnO4- + 4H+ +3e-
b) Account for the following:
2,3
(i) Zn is not considered as a transition element.
(ii) Transition metals form a large number of complexes.
(iii)
The Eo value for the Mn3+/Mn2+ couple is much more positive than that for Cr3+/Cr2+
couple.
Or
(i)
With reference to structural variability and chemical reactivity, write the differences
between lanthanoids and actinoids.
(ii)
Name a member of the lanthanoids series which is well known to exhibit +4 oxidation
state.
(iii)
Complete the following equation :
MnO4- + 8H+ + 5e-
(iv)
Out of Mn3+ and Cr3+ , which is more para magnetic and why ?
(At. No. : Mn=25, Cr=24 )5
2015
1. MnO is basic whereas Mn2O7 is acidic in nature. Why?
2. Transition metals form alloys. Why?
3. Complete the following equation : 2MnO2 + 4 KOH +O2 
4. Why do actinoids show wide range of oxidation states ?
5. Why is actinoid contraction greater than lanthanoid contraction?
2016
Account for the following:
a) Mn2O7 is acidic whereas MnO is basic
b) Zr & Hf exhibit similar properties
c) Transition metals form a large number of complex compounds
A) Write the preparation of K2MnO4 from pyrolusite ore (MnO2)
B) Write the type of magnetism shown by KMnO4 and K2MnO4
C) The elements of 3d transition series are given as : Sc Ti V Cr Mn Fe Co Ni Cu Zn
Answer the following:
1. Cu has exceptionally positive E0 ( M2+/M) value. Why
2. Which element is a strong reducing agent in +2 oxidation state and why?
3. Zn 2+ salts are colorless Why?
B. Write the preparation of sodium dichromate from chromite ore( FeCr2O4)
1. Account for the following
a) Transition metals show variable oxidation states
b) Zn, Cd, Hg are soft metals
c) E0 values for the Mn3+ / Mn2+ couple is highly positive ( + 1.57 V) as compare to Cr3+/ Cr2+
2. Write one similaty and one difference between the chemistry of lanthanoid and actinoid
elements.
3. Following are the transition metal ions of 3D series :
Ti4+ , V2+ , Mn2+ , Cr3+
Answer the following questions
a) Which ion is the most stable in an aqueous solution and why ?
b) which ion is a strong oxidizing agent and why ?
c) which ion is colourless and why
4. Complete the following equations
a) 2 MnO4 - + 16 H+ + 5 S2- 
b) KMnO4 + heat 
2017
2018
1. Complete and balance the following chemical equations :
(a) Fe2+ + MnO4– + H+ →
(b) MnO4– + H2O + I– →
2. Give reasons :
(a) Eº value for Mn3+/Mn2+ couple is much more positive than that for Fe3+/Fe2+.
(b) Iron has higher enthalpy of atomization than that of copper.
(c) Sc3+ is colourless in aqueous solution whereas Ti3+ is coloured.
2019
Explain the method of preparation of sodium dichromate from chromite ore. Give the equation
representing oxidation of ferrous salts by dichromate ion.
Coordination Compounds
U-9
2007
Describe the type of hybridization, shape and magnetic property for the following ions
1. [Fe(H2O)6]2+
2008
2. [Co(NH3)6]3+
3. [NiCl4]2-
1. What is the basis of formation of the spectrochemical series?
2. Draw geometrical isomers for
a) [Co(NH3)3Cl3]
2009
b) [CoCl2(en)2]2+
1. Explain with example
a) Crystal field splitting
b) Linkage isomerism
c) Ambidentate ligand
2. Describe the type of hybridization, shape and magnetic property for the following
a) [Co(NH3)6]3+
b) [Cr(NH3)6]3+
c) [Ni(CO)4]
3. Explain
i.
Low spin octahedral complexes for Ni are not known
ii.
The π- complexes are known for transition elements only
iii.
CO is a stronger ligand than NH3 for many metals
4. . Describe the type of hybridization, shape and magnetic property for the following
a) [Ni(CN)4]22010
b) [NiCl4]2-
c) [CoF6]3-
1. Explain
i.
Low spin octahedral complexes for Ni are not known
ii.
The π- complexes are known for transition elements only
iii.
Co2+ is readily oxidises to Co3+ in the presence of a strong ligand
2. Describe the type of hybridization, shape and magnetic property for the following
[CoCl4]2- , [Ni(CN)4]2- , [Cr(H2O)2(C2O4)2]-
2011
1. Explain with example
a) Crystal field splitting in an octahedral field
b) Denticity of a ligand
c) Ambidentate ligand
2. Write structure and name of the stereo isomers of :
i.
[Co(en)3]Cl3 ii. [Pt(NH3)2Cl2]
iii. [Fe(NH3)4Cl2]Cl
3. Describe the type of hybridization, shape and magnetic property for the following
[Cr(NH3)4Cl2]Cl
2012
,
[Co(en)3]Cl3 , K2[Ni(CN)4]
1. Name the following compounds and draw the structure of their stereo isomer
a) [Co(en)2Cl2]+
b) [Cr(C2O4)3]3-
c) [Co(NH3)3Cl3]
2. Name the following and describe their structure
a) [Fe(CN)6]42013
b) [Cr(NH3)4Cl2]+
c) [Ni(CN)4]2-
(a) For the complex [NiCl4]–2, write
(i) The IUPAC name
(ii) The hybridization type
(iii) The shape of the complex
(Atomic no. of Ni = 28)
(b) What is meant by crystal field splitting energy ? On the basis of crystal field theory, write the electronic
configuration of d4 in terms of t2g and eg in an octahedral field when
(i) Δ0 > P
2014
(ii) Δ0 < P
1) (i) Write the IUPAC name of the complex [Cr(NH3)4Cl2]Cl.
3
(ii) What type of isomerism is exhibited by the complex [Co(en)3]3+?
(en =ethane-1,2-diamine)
(iii) Why is[NiCl4]2- paramagnetic but [Ni(CO)4] is diamagnetic?
(At No. : Cr=24,Co=27,Ni=28)
2015
a) Write down IUPAC name of the following complex : K3[Fe(CN)6]
b) Write the formula for the following complex : Pentaamminenitrito-N-cobalt(III)
c) What type of isomerism is shown by the complex [Ag(NH3)2][Ag(CN)2] ?
d) On the basis of crystal field theory , write the electronic configuration for d4 ion if Δo < P.
e) Write the hybridization and shape of [Ni(CN)4]2- , (atomic number of Ni = 28 )
2016
1. When a coordination compound PtCl4.6NH3 is mixed with AgNO3, 4 moles of AgCl are precipitated per mole of the
compound. Write
a) Structural formula of the complex
b) IUPAC name of the complex
2. For the complex [CoF6]3- , write the hybridization type, magnetic character and spin nature of the complex. (
Atomic no of Co = 27)
3. Why is the complex [Co(en)3]3+ more stable than the complex [CoF6]3- ?
2017
1. Using IUPAC norms write the formulae a) Sodium dicyanidoaurate(I)
a) Tetraamminechloridonitrito-N-platinum(IV) sulphate
2. Using IUPAC norms write the formulae a) Tris(ethane-1,2-diamine)chromium(III) chloride
Potassium tetrahydroxozincate(II)
b)
3. Using IUPAC norms write the formulae a) Dichloridobis(ethane-1,2-diamine)cobaltIII)
b) Potassium
trioxalatoaluminate(III)
4. What type of isomerism is shown by the complex [Co(NH3)5 (SCN)]2+
5. Why is [NiCl4]2- paramagnetic while [Ni(CN)4]2- is diamagnetic ?
Why are low spin tetrahedral complexes rarely observed ?
2018
1. Write the coordination number and oxidation state of Platinum in the complex [Pt(en)2Cl2].
2.(a) Write the formula of the following coordination compounds: Iron(III)Hexacyanoferrate(II)
(b) What type of isomerism is exhibited by the complex [Co(NH3)5Cl]SO4 ?
(c) Write the hybridisation and number of unpaired electrons in the complex [CoF6]3–
(Atomic No. of Co = 27)
2019
When a coordination compound CrCl3 . 6H2O is mixed with AgNO3, two moles of AgCl are precipitated per
mole of the compound. What is the structural formula of the coordination compound ?
What is the difference between a complex and a double salt ?
Organic Chemistry (2007-2019)
U-10-13
IUPAC
name
1. CH3COCH2COCH3
2. CH3OCH2CH(CH3)CH2CH3
3. H2C=CH-CH(OH)-CH2CH2CH3
4.
5. CH2=CH-CH2Br
6.
7.
8.
9. CH3-C(CH3)2-CH(Cl)-CH3
10. C6H5-CH2-CH(OH)-CH3
1. Write the IUPAC name of : CH3-C(CH3)=C(Br)-CH2-OH
2. Write the IUPAC name of : C6H5 – CH=CH-CH2-OH
3. Write the IUPAC name of :
CH3
H3C
O
C
CH3
CH3
11.
12.
13.
14.
Structure
Reasoning
1.
2.
3.
4.
5.
6.
7.
8.
4-chloropentan-2-one
1-phenylpentan-1-one
1-phenylpropan-2-ol
2,2-dimethylphenol
Write the structure of 2-aminotoluene
n-methylethanamine
4-chloropentan-2-one.
p-methylbenzaldehyde
1. Amines react as nucleophiles
2. Amine are basic while amides are neutral
3. Nitro compounds have high b.pt than hydrocarbons
4. Aromatic amines are weaker base than aliphatic amines
5. Haloalkes are more reactive towards SN reactions than haloarenes
6. Phenols do not give protonation reaction easily.
7. pKb value for aniline is more than that for methyl amine.
8. Methyl amine in water reacts with ferric chloride to give ppt of ferric hydroxide
9. Aniline does not undergo Friedel Craft reaction.
10. The bpt of ethanol is higher than methoxymethane
11. Ethylamine is soluble in water but aniline is not.
12. Primary amines have higher bpt than tertiary amine.
13. Alcohols are more soluble in water than hydrocarbon.
14. Ortho-nitro phenol is more acidic than ortho-methoxy phenol
15. Ethanal is soluble in water. Why ?
16. Ethyl iodide undergoes N2 S reaction faster than ethyl bromide.
17. (±) 2-Butanol is optically inactive.
18. C -X bond length in halobenzene is smaller than C -X bond length in CH3 – X.
Primary amines(R-NH2) have higher boiling point than tertiary amines(R3N).
(i)
Aniline does not under go Friedel craft reaction.
(ii)
(CH3)2NH is more basic than (CH3)3N in an aqueous solution.
19.
20.
21.
22.
23.
Cl-CH2COOH is a stronger acid than CH3COOH
Carboxylic acids do not give reaction of carbonyl group
Benzyl chloride is highly reactive towards the SN1 reaction
2-bromobutane is optically active but 1-bromobutane is optically inactive
Electrophilic reactions in haloarenes occur slowly.
Conversio
n
24.
4. Give reasons :
a) Acetylating of aniline reduces its activation effect
b) CH3NH2 is more basic than C6H5NH2
c) Although –NH2 is o/p directing group , yet aniline on nitration gives a significant amount of mnitroaniline
Out of chlorobenzene and benzyl chloride, which one gets easily hydrolysed by aqueous NaOH and why
?(2018)
(a) Aromatic carboxylic acids don not undergo Friedel-Crafts reaction.
(b) pKa value of 4-nitrobenzoic acid is lower than that of benzoic acid.
(i) (CH3)2NH is more basic than (CH3)3N in an aqueous solution
(ii) Aromatic diazonium salts are more stable than aliphatic diazonium salts.
Why is t-butyl bromide more reactive towards SN1 reaction as compared to n-butyl bromide ?
Propanamine and N,N-dimethylmethanamine contain the same number of carbon atoms, even though
Propanamine has higher boiling point than N,N-dimethylmethanamine. Why ?
Give reasons for the following : (a) The presence of –NO2 group at ortho or para position increases the
reactivity of haloarenes towards nucleophilic substitution reactions. (b) p-dicholorobenzene has higher
melting point than that of ortho or meta isomer. (c) Thionyl chloride method is preferred for preparing alkyl
chloride from alcohols
Why aniline does not undergo Friedel-Crafts reaction ?
1. Ethanol to 3-hydroxybutanal
Benzaldehyde to benzophenone
2. Propanone to propen
Benzoic acid to benzaldehyde
3. Bromobenzene to 1-phenylethanol
Phenol to benzoquinone
4. Propanone to 2-methylpropan-2-ol
Propene to propan-2-ol
5. Cyclohexanol to cyclohexan-1-one
6. Ethyl benzene to benzoic acid
7. Bromobenzene to benzoic acid
8. Ethyl cyanide to ethanoic acid
9. Methyl benzene to benzoic acid
10. Ethanol to ethane
11. Methyl magnesium bromide to 2-methylpropan-2-ol
12. Propene to propan-2-ol
13. Ethanol to but-2-enal
14. Butanol to butanoic acid
15. Butan-1-ol to butanoic acid
16. 4-methylacetophenone to benzene-1,4-dicarboxylic acid
17. Propanone to Propan-2-ol
18. Ethanal to 2-hydroxy propanoic acid
19. Toluene to benzoic acid
20. Aniline to phenol
21. Prop-1-ene to Propan-1-ol
22. Anisole to 2-methoxytoluene
23.
5. How will you convert the following in not more than two steps
a) Benzoic acid to Benzaldehyde b) Acetophenone to Benzoic Acid
c) Ethanoic acid to 2-Hydroxyethanoic acid.
Name
Reactions
(a) Ethanal to Propanone
(b) Toluene to Benzoic acid
Carry out the following conversions : (i) P-nitrotoluene to 2-bromobenzoic acid (ii) Propanoic acid to acetic
acid
Carry out the following conversions : (i) Benzoic acid to aniline (ii) Bromomethane to ethanol
1. Rosenmund Reduction
2. Cannizzaro Reaction
3. Fischer Esterification
4. Hofman’s bromamide reactions
5. Grabiel phthalimide synthesis
6. Acetylation
7. Decarboxylation
8. HVZ Reaction
9. Clemmensen reaction
10. Wolff-Kishner Reduction
11. Carbyl amine reaction
12. (i) Reimer – Tiemann reaction
(ii) Williamson’s ether synthesis
(i)
Rosenmund reduction
(ii)
Cannizzaro’s reaction
(i)
(ii)
Distinguis
h
Reimer – Tiemann reaction
Williamson synthesis
6. Write the reactions involved in gth efollowing
a) Etard reaction b) Stephen reduction
Write the reactions involved in the following,
(i) Hofmann bromamide degradation reaction
(ii) Diazotisation
(iii) Gabriel phthalimide synthesis
Write the reaction involved in the Hoffmann bromamide degradation reaction.
Define with equation : (a) Riemer-Tiemann Reaction (b) Williamson’s Synthesis
1. Propanal and propanone
2. Phenol and benzoic acid
3. Acetophenone and benzophenone
4. Ethanal and propanal
5. Benzoic acid and ethyl benzoate
6. Ethyl amine and aniline
7. Aniline and benzyl amine
8. Methyl amine and di methyl amine
9. Aniline and N-methylaniline
10. Benzaldehyde and acetophenone
11. Propanol and propanone
12. Pentan-2-one and Pentan-3-one
13. Ethanal and Propananl
Benzonoic acid and Phenol
1. (ii) Propanal and Propanone
2. C6H5-NH2 and CH3-NH2
3.
7. Give simple tests to distinguish between the following pairs of compounds :
a) Butanal and Butan-2-one b) Benzoic acid and Phenol
Give a simple chemical test to distinguish between Aniline and N,N-dimethylaniline.
Other
questions
1. What are chiral objects? Is there any chirality in 3-bromopent-1-ene?
2. Which one will give SN1 faster and why?
3. Write the reagent and reaction to prepare i) ethoxybenzene ii) 2-methyl-2-methoxypropane by
Williamson synthesis
4. Write a chemical reaction in which iodide ion displaces diazonium group from diazinium salt.
5.
6.
7.
8.
9.
10.
11.
What is Tollen’s reagent? Write one usefulness of this reagent.
How would you differentiate SN1 and SN2 mechanism. Give one example of each.
Explain the mechanism of acid catalysed hydration of alkene to corresponding alcohol.
What is meant by chirality of a compound. Give example.
Which one is more easily hydrolysed by aq KOH and why : CH3CHClCH2CH3 , CH3CH2CH2Cl
In the following pair of halogen compounds, which would undergo SN2 reaction faster and why?
12.
13.
14. Which acid is more stronger?
a) F-CH2-COOH or Cl-CH2-COOH
b) C6H5OH or CH3-COOH
14. Which will undergo SN2 reaction faster ?
CH3-CH(CH3)-CH2-CH2-Br and CH3-CH2-CH(CH3)-CH2-Br
(a) Out of CH3CH2-CO-CH2-CH3 and CH3CH2- CH2-CO-CH3, which gives idoform test?
(b) Which Halogen compound in each of the following pairs will react faster in SN2 reaction :
(i) CH3Br or CH3-Cl
(ii) (CH3)3C-CL or CH3-Cl
1) (a)Draw the srtucre of the Major monohaloproducts in each of the following :
1) Identify the chiral molecule in the following pair:
1
The conversion of primary aromatic amine into diazonium salts is Known as ________________.
X
X
1. Out of
and
, which is an example of allylic halaide ?
X
X
2. Out of
and
, which is an example of vinylic halaide ?
CH2Cl
3. Out of
CH2CH2Cl
and
, which is an example of a benzylic halide ?
8. Write the mechanism ( using curved arrow notation ) of the following reaction
H3O +
H2C
CH2
H3C
+
CH2
+ H2O
9. Write the structures of the products when Butan-2-ol reacts with the following : a) CrO3 , b)
SOCl2
10. The following compound are given to you : 2-Bromopentane, 2-Bromo-2-methylbutane, 1Bromopentane
a) which one is most reactive towards SN2 reaction?
b) which one is optically active
c) write the compound which is most reactive towards β-elimination reaction
Complete
the rkn
1. C6H5N2Cl + KI 
2. CH2=CH2 + Br2 
3. CH3CH2-CH=CH2 + HBr 
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
RCONH2 + LiAlH4/H2O 
C6H5N2Cl + CH3COCl 
C2H5NH2 + C6H5SO2Cl 
C2H5NH2 + HNO2 
CH3-CH2-Cl + NaCN  A
C6H5-NH2 + NaNO2/HCl  A
A + H2/Ni  B
( identify A & B )
A + C6H5NH2  B ( identify A & B )
Complete each synthesis by giving missing starting material, reagent or products
15. CH2=CH-CH2-CCH + Br2 
1. CH3CH2NH2 + CHCl3 + alc KOH 
2. C6H5N2+Cl- + H2O 
3. C6H5NH2 + HCl(aq) 
4. C6H5COOH + Br2/FeBr3 
Name the reagent used in the following reaction :
a) C6H5-COCl  C6H5-CHO
b) CH3-COONa  CH4
Complete :
(i) CH3-CHO + HCN 
(ii) C6H5-MgBr + CO2 + H3O+ 
(iii) CH3-CN + LiAlH4 
2) Write the Products formed when CH3CHO reacts with the following reagents:
(i)
HCN
(ii)
H2N-OH
CH3CHO in the presense of dilute NaOH.
Give the structures of A,B and C in the following reactions:
(i)
C6H5NO2 ---Sn+HCl---->A----NaNO2+HCl/273K---->B----H2O---->C
CH3CN -----H2O/H+----->A -----NH3/Δ------>B -----Br2 + KOH---->C
1) Write the equation involved in the following reactions:
2) Write the mechanism of the following reaction :
CH3CH2OH -----(HBr)----> CH3CH2Br +H2O
What happens when
a) ethanol is treated with Cu at 573 K
b) phenol is tyrated with CH3COCl/anhydrous AlCl3
2
2
c) ethyl chloride is treated with NaOCH3
Write the structures of A,B,C,D&E
C6H5NH2+CH3COCl+pyridineA  + Br2/CH3COOHB+H+ C
C6H5NH2 +CHCl3+KOHD
A+HNO3+H2SO4E
Write the structures of main products when benzene diazonium chloride reacts with the following reagents :
a) KI b) CH3CH2OH c) Cu/HCl
(b) Write the structure of the product when chlorobenzene is treated with methyl chloride in the presence of
sodium metal and dry ether.
(c) Write the structure of the alkene formed by dehydrohalogenation of 1-bromo-1-methylcyclohexane with
alcoholic KOH
Arrange
1.
2.
3.
4.
C6H5NH2, (C2H5)2NH , (C2H5)3N and NH3 (increasing base strength in water)
C2H5NH2, (C2H5)2NH , (C2H5)3N and CH3NH2 (increasing base strength in gas phase)
NH3, CH3NH2 , (CH3)2NH , (CH3)3N (increasing base strength in aqueous soln)
CH3CH2CH(Br)COOH, CH3CH(Br)CH2COOH, (CH3)2CHCOOH , CH3CH2CH2COOH
(acid strength)
5. Benzoic acid, 4-Nitrobenzoic acid, 3,4-Dinitrobenzoic acid, 4-Methoxybenzoic acid (acid strength)
6. C6H5NH2, C6H5N(CH3) , (C6H5)2NH , CH3NH2 ( increasing base strength)
7.
Arrange the compounds of each set in order of reactivity towards SN2 displacement:
(i) 2-Bromo-2-methylbutane, 1-Bromopentane, 2-Bromopentane
(ii) 1-Bromo-3-methylbutane, 2-Bromo-2-methylbutane, 3-Bromo-2-methylbutane
(iii) 1-Bromobutane, 1-Bromo-2,2-dimethylpropane, 1-Bromo-2-methylbutane, 1-Bromo-3-methylbutane.
Arrange according to increasing order of bp: CH3CHO, CH3CH2OH, CH3-CH2-CH3
Arrange according to increasing reactivity towards nucleophilic addition : CH3COCH3,C6H5-CO-C6H5, CH3CHO
Arrange according to increasing acidic character : Cl2CH-COOH , Cl-CH2-COOH , CCl3-COOH
Increasing basic character in aq solution : CH3NH2 , (CH3)2NH , (CH3)3N
1. Arrange the following compounds in the increasing order of their acid strength : p-cresol, pnitrophenol, phenol
2. Arrange the following in the increasing order of their pKb values. :
C6H5NH2, C2H5NH2, C6H5NHCH3
An organic compound contains 69.77% carbon, 11.63% hydrogen and rest oxygen.
The molecular mass of the compound is 86. It does not reduce Tollens’ reagent
but forms an addition compound with sodium hydrogensulphite and give positive
iodoform test. On vigorous oxidation it gives ethanoic and propanoic acid. Write
the possible structure of the compound.
(A), (B) and (C) are three non-cyclic functional isomers of carbonyl compound with molecular formula
C4H8O.
Isomers (A) and (C) give positive Tollens’ test whereas isomer (B) does not give Tollens’ Test but gives
positive
Iodoform test. Isomers (A) and (B) on reduction with Zn(Hg)/cons.HCl give the same product (D).
(a) Write the structures of (A), (B), (C) and (D)
(b) Out of (A), (B) and (C) isomers, which one is least reactive towards addition of HCN ?
An alkene with molecular formula C5H10 on ozonolysis gives a mixture of two compounds, B and C.
Compound B gives positive Fehling test and also reacts with iodine and NaOH solution. Compound C does
not give Fehling solution test but forms iodoform. Identify the compounds A, B and C.
U2007
2008
2009
Biomolecules
What are reducing sugars?
What is meant by denaturation of a protein?
Define enzyme
Write two main functions of carbohydrate in plants
What happens when glucose is treated with
i) HI ii) Bromine water iii) HNO3
How are vitamins classified? Mention the chief source of Vitamin A and C
Describe by giving example
i) Glycosidic linkage ii) Peptide linkage iii) Primary structure of protein iv)
Denaturation of protein.
Name the four bases in DNA. Which one is not present in RNA?
Name two fat soluble vitamins, their sources and diseases caused due to their deficiency
2010
What are reducing sugars?
Amino acids may be acidic,alkaline or neutral. How does this happen?
What are essential and non essential amino acids? Name one of each type.
What are the product of hydrolysis of sucrose?
Differentiate between fibrous and globular proteins.
What is meant by denaturation of a protein?
What are mono saccharides ?
2011
1. Explain
i) Peptide linkage ii) Pyranose structure of glucose
2. Write the main structural difference between DNA and RNA
3. Of the four bases , name those which are common to both DNA and RNA
4. Write such reactions and facts about glucose that cannot be explained by its open
chain structure.
2012
What is essentially the difference between -glucose and -glucose ?
What is meant by pyranose structure of glucose ?
Write the structure of product obtained when glucose is oxidised by nitric acid.
(a) Write the name of linkage joining two amino acids.
(b) Shanti, aa domestric helper of Mrs. Anuradha, fainted while mopping the floor. Mrs.
Anuradha immediately took her to the nearby hospital where she was diagnosed to be
severely ‘anaemic.’ The doctor prescribed an iron rich diet and multivitamins
supplement to her. Mrs. Anuradha supported her financially to get the medicines.
After a month, Shanti was diagnosed to be normal.
After reading the above passage, answer the following questions :
(i) What values are displayed by Mrs. Anuradha ?
(ii) Name the vitamin whose deficiency causes ‘pernicious anaemia’.
(iii) Give an example of waer soluble vitamin.
2013
What is the product of hydrolysis of sucrose?
2014
2015
1) What are the products of hydrolysis of sucrose?
1
2) Define the following terms as related to protiens:
3
(i)
Peptide linkage
(ii)
Primary structure
(iii)
Denaturation
3) What are the products of hydrolysis of maltose?
1
4) Define the following terms:
3
(i)
Glycosidic linkage
(ii)
Invert sugar
(iii)
Oligosaccharides
1. Which one of the following is an oligosaccharide : starch, maltose,fructose,glucose?
2. Write one difference between DNA and RNA?
3. Write the name of the disease caused by the deficiency of Vitamin B1
2016
2017
2018
2019
U-
After watching a programmme on TV about the presence of carcinogens ( cancer causing
agents) Potassium bromated and Potassium iodate in bread and othe bakery products ,
Rupali a class XII student decided to make others aware about the adverse effects of
these carcinogens in food. She consulted the school principal and requested him to
instruct the canteen contractor to stop selling sandwiches, pizzas, burgers and othe
bakery products to the students. The principal took an immediate action and instructed
to the canteen contractor to replace the bakery products wit some protein and vitamin
rich food like fruits , salads, sprouts , etc. The decision was welcome by the parents and
the students.
After reading the above passage , answer the following questions :
a) What are the values ( at least two ) displayed by Rupali ?
b) Which polysaccharide component of carbohydrate is commonly present in bread ?
c) Write the two types of secondary structures of protein
d) Give two examples of water soluble vitamins.
1.Define the following with an example of each :
(a) Polysaccharides
(b) Denatured protein
(c) Essential amino acids
2.(a) Write the product when D-glucose reacts with conc. HNO3?
(b) Amino acids show amphoteric behaviour. Why ?
(c) Write one difference between α-helix and β-pleated structures of proteins.
(a) Give any one property of glucose that cannot be explained by the open chain structure.
(b) Compare amylase with amylopectin in terms of constituting structure. (c) Why do
amino acids show amphoteric behaviour ?
(a) What is the difference between native protein and denatured protein ? (b) Which one of
the following is a disaccharide : Glucose, Lactose, Amylose, Fructose (c) Write the name
of the vitamin responsible for the coagulation of blood.
Polymer
2007
Write formula of monomer of polythene and Teflon
2008
Define the term polymerization
What are thermoplastic and thermosetting polymer. Give examples
Distinguish between homo polymer and co polymer with examples
What does 6 ,6 indicates in Nylon-6 6?
What are thermoplastic and thermosetting polymer. Give differences and examples
What is the primary structural features necessary for a molecule to make it useful in a condensation
polymerization reaction?
Differentiate condensation and addition polymerization with examples
2009
2010
What does 6 ,6 indicates in Nylon-6 6?
Draw the molecular structure and write the name of monomer of i) PVC ii) Teflon
What is meant by co polymerization?
Draw the molecular structure and write the name of monomer of i) Bakelite ii) Nylon-6
2011
Draw the molecular structure and write the name of monomer of i) PVC ii) Teflon iii) Polythene
iv) Buna-S v) Dacron vi) Neoprene
2012
2013
Differentiate between thermoplastic and thermosetting polymer. Give examples.
1. Give one example of a condensation polymer.
2. Define thermoplastic and thermosetting polymers. Give one example of each.
3. What is a biodegradable polymer ? Give an example of a biodegradable aliphatic polyester.
4. Is (-CH2-CH(Cl))n a homopolymer or copolymer?
1) Which of the following is natural polymer?
1
Buna-S, Proteins, PVC
2) Write the name of monomers used for getting the following polymers: 2
(i)
Bakelite ii) Neoprene
3) Based on molecular forces what type of polymer is neoprene?
1
4) Write the name of monomers used for getting the following polymers: 2
(i)
Terylene ii) Nylon-6,6
1. Write the names and structures of the monomers of the following polymers :
a) Glyptal b) Teflon c) Nylon-6
1. Write the names and structures of the monomers of the following polymers :
a) Buna-S b) Terylene c) Nylon-6
Write the structures of the monomers used for getting the following polymers :
a) Nylon -6,6 b) Melamine –formaldehyde polymer c) Buna-S d) Polyvinyl chloride (PVC) e)
Buna-N f) Teflon g) Neoprene
Shyam went to a grocery shop to purchase some food items. The shopkeeper packed all the item in
polythene bags and gave them to Shyam. But Shyam refused to accept the polythese bags and asked
the shopkeeper to pack the items in paper bags. He informed the shopkeeper about the heavy penalty
imposed by the
government for using polythene bags. The shopkeeper promised that he would use paper bags in
future in place of polythene bags.
Answer the following :
(a) Write the values (at least two) shown by Shyam
(b) Write one structural difference between low-density polythene and high-density polythene
(c) Why did Shyam refuse to accept the items in polythene bags ?
(d) What is a biodegradable polymer ? Give an example.
Give the structures of monomers of the following polymers : (a) Nylon-6,6 (b) Buna-S
Classify the following as addition and condensation polymers giving reason : (a) Teflon (b) PHBV
2014
2015
2016
2017
2018
2019
Write the name of monomers and their structures for the following polymers : (a) Neoprene (b)
Nylon-6
U-16
2008
2009
2010
2011
2012
2013
Chemistry in everyday life
Mention one use the following drugsi) Ranitidine ii) Paracetamol ii) Tincture of iodine
Describe with example i) Non ionic detergent ii) Food preservatives iii) Disinfectants iv) cationic detergent
v) Enzymes vi) sweetening agents
Describe with example
i) detergent ii) Food preservatives iii) enzymes iv) antibiotic v) antiseptic vi) analgesic
What are analgesic drugs? How are they classified and when they usually recommended for use.
Describe with examplei) synthetic detergent ii) Food preservatives iii) antacids
Differentiate between disinfectant and antiseptic.What are food preservative ? Name two such substances.
(i) What class of drug is Ranitidine ?
2014
(ii) If water contains dissolved Ca2+ ions, out of soaps and synthetic detergents, which will you use for cleaning
clothes ?
(iii) Which of the following is an antiseptic ? 0.2% phenol, 1% phenol
1) On the occasion of World Health Day, Dr. Satpal organized a ‘health camp’ for the poor farmers living in a
nearby village. After checkup, he was shocked to see that the most farmers suffered from cancer due to
regular exposure to pesticides and many were diabetic. They distributed free medicines to them. Dr. Satpal
immediately reported the matter to the National Human Rights Commissions (NHRC). On the suggestion
of NHRC, the govt. decided to provide medical care, financial assistance, setting up of super specialty
hospitals for treatment and prevention of the deadly disease in the affected village all over the India.
2015
(i)
Write the values shown by a) Dr. Satpal b) NHRC
(ii)
What type of analgesics are chiefly used for the relief of pains of terminal cancer?
(iii)
Give an example of artificial sweetener that could have been recommended to diabetic patients.
Mr Roy the principal of one reputed school organized a seminer in which he invited parents and principals to
discuss the serious issue of diabetes and depression in students. They all resolved this issue by strictly banning junk
food in schools and introducing healthy snacks and drinks like soup, lasssi, milk etc in school canteens. They also
decided to make compulsory half an hour of daily physical activities for the students in the morning assembly. After
six months, Mr Roy conducted the health survey in most of the schools and discovered a tremendous improvement
in the health of the students.
(i) What are the values (at least two) displayed by Mr Roy?
(ii) As a student , how can you spread awareness about this issue ?
(iii) What are tranquilizers? Give an example. (iv) Why is use of aspartame limited to cold foods and drinks ?
2016
2017
2018
2019
Define the following a) Anionic detergents b) Limited spectrum antibiotics c) Antiseptics d) Antacids
e) Narrow spectrum antibiotics , f) Cationic detergents g) Broad spectrum antibiotics h) Tranquilizers
(a) Why is bithional added to shop ?
(b) What is tincture of iodine ?write its one use.
(c) Among the following, which one acts as a food preservative ?
Aspartume, Asprin, Sodium Benzoate, Paracetamol
Define the following with suitable example of each : (a) Antiseptics (b) Non-narcotic analgesics (c) Cationic
detergents