Q. BANK – ACID BASE AND SALT
Q.
Write the balanced equations for the preparation of the following compounds (as the
major product) starting from iron and using only one other substance:
(i) Iron (II) chloride (ii) Iron (III) chloride (iii) Iron (II) sulphate (iv) Iron (II) sulphide.
Q.
Copy and complete the following table – Column 3 has the names of the gases to be
prepared using the substance you enter in Column 1 along with dilute or concentrated
Sulphuric acid as indicated by you in Column 2.
Column 1
Column 2
Column 3
Substance
reacted
Dilute or concentrated
with acid
Gas Sulphuric
acid
Hydrogen
Q.
Write the equations for the laboratory preparation of :
(i) Sodium sulphate using dilute Sulphuric acid.
(ii) Lead sulphate using dilute Sulphuric acid.
Q.
Write the equation for the laboratory preparation of the following salts using sulphuric
acid:
(i) Iron II sulphate from iron.
(ii) Copper sulphate from copper.
(iii) Lead sulphate from lead nitrate.
(iv) Sodium sulphate from sodium carbonate.
Q.
Choosing the correct words given in brackets, complete the sentences given below:
(i) An acid is a compound which when dissolved in water gives ________
(hydronium/hydroxide) ions as the only ________ (positive/negative) ions.
(ii) An _________ (acid/basic) salt is one in which the hydrogen of an acid has
been partially replaced by a _________ (metal/non-metal).
Q.
Which of the following methods, A, B, C, D, or E is generally used for preparing the
chlorides listed below from (i) to (v). Answer by writing down the chloride and the letter
pertaining to the corresponding method. Each letter is to be used only once.
A. Action of an acid on a metal.
B. Action of an acid on oxide or carbonate.
C. Direct combination.
D. Neutralization of an alkali by an acid.
E. Precipitation (double decomposition).
(i) Copper (II) chloride.
(ii) Iron (II) chloride.
(iii) Iron (III) chloride.
(iv) Lead (II) chloride.
(v) Sodium chloride.
Q.
Fill in the blanks with suitable words:
An acid is a compound which when dissolved in water form Hydronium ions as the only
(i) ___________ ions. A base is a compound which if soluble in water contains (ii)
____________ ions. A base reacts with an acid to form a (iii) _________ and water only.
This type of reaction is known as (iv) _________ .
.
Q.
The preparation of Lead sulphate from Lead carbonate is a two-step process. (Laed
sulphate cannot be prepared by adding dilute Sulphuric acid to Lead carbonate.)
(i) What is the first step that is required to prepare Lead sulphate from Lead carbonate ?
(ii) Write the equation for the reaction that will take place when this first step is carried
out. (iii) Why is the direct addition of dilute sulphuric acid to Lead carbonate an
impractical method of preparing Lead sulphate?
Q.
(i) Which feature of the Ammonia molecule leads to the formation of the
Ammonium ion when Ammonia dissolves in water?
(ii) Name the other ion formed when Ammonia dissolves in water.
(iii) Give one test that can be used to detect the presence of the ion produced
in(ii).
Q.
Match the descriptions below with the appropriate term from the list A to F: A: Acidic oxide, B: Alkali, C: Amphoteric oxide, D: Basic oxide,
E: Deliquescence, F: Efflorescence.
(i) The property of spontaneously giving up water of crystallization to the
atmosphere. (ii) A compound, soluble in water and the only negative ions in the
solution are hydroxide ions.
Q.
What is observed when, neutral litmus solution is added to sodium hydrogen
carbonate solution.
Q.
Acids dissolve in water to produce positively charged ions. Draw the structure
of these ions.
Q.
Mention the colour changes observed when the following indicators are added
to acids :(i) Alkaline phenolphthalein solution.
(ii) Methyl orange solution.
(iii) Neutral litmus solution.
Q.
Which of the following hydroxides is not an alkali :–
(a) ammonium hydroxide (b) calcium hydroxide
(c) copper hydroxide (d) sodium hydroxide.
Q.
From the list given below, select the word(s) required to correctly complete blanks (i) to
(v) in the following passage :ammonia, ammonium, carbonate, carbon dioxide, hydrogen, hydronium, hydroxide,
precipitate, salt, water.
A solution X turns blue litmus red, so it must contain (i) ---------- ions; another solution Y
turns red litmus blue and therefore, must contain (ii) ------------- ions. When solution X
and Y are mixed together, the products will be a (iii) ------------- and (iv) ------------- . If a
piece of magnesium were put into solution X, (v) -------------- gas would be evolved.
Q.
Match the following :Column A
Column B
1. Acid salt
A. Sodium potassium
carbonate
2. Mixed salt
B. Alum
3. Complex salt
C. Sodium carbonate
4. Double salt
D. Sodium zincate
5. Normal salt
E. Sodium hydrogen carbonate
Q.
From the list of the substances given below, choose the pair required to prepare the salts
(i) to (iii) in the laboratory and write down the relevant equations.
The substances are :
Iron, Chlorine, Lead Nitrate solution, Sodium Nitrate solution, Iron (III) Carbonate,
Lead Carbonate, Iron (III) Hydroxide, Sodium Hydroxide and dilute Hydrochloric acid.
(i) Sodium Chloride (ii) Lead Chloride (iii) Anhydrous Iron (III) Chloride.
Q.
All Ammonium salts are decomposed on heating. What other property do Ammonium
salts have in common?
Q.
Answer the following questions, relating your answers only to salts in the list given below
:
Anhydrous Calcium Chloride, Copper Sulphate-5-water, Sodium Carbonate-10 – water.
(a) Which compound is efflorescent?
(b) Which compound is blue in colour?
(c) Which compound is deliquescent?
(d) What would be seen on mixing a solution of Calcium chloride with a solution of
Sodium carbonate?
(e) Write the balanced equation for occurring when a solution of Calcium chloride is
mixed with a solution of Sodium carbonate.
Q.
In this question, you are required to supply the word (or words) that will make the
following sentence into correct statement which is to be written down in full.
Calcium nitrate reacts with Sodium sulphate to form Calcium sulphate.
Q.
Describe in each case, one chemical test that would enable you to distinguish between the
following pairs of chemicals. Describe what happens with each chemical or state “no
visible reason”.
(a) Sodium chloride solution and sodium nitrate.
(b) Sodium sulphate solution and Sodium chloride solution.
Q.
Write balanced equations for each of the following reactions :
(a) Action of heat on Copper nitrate. (b) Zinc and dilute Sulphuric acid.
Q.
(a) Choose the correct word or phrase from the brackets to complete the following
sentences :
(i) Ammonium chloride is a soluble salt prepared by (precipitation, neutralization).
(ii) When Ammonium chloride is heated, it undergoes (thermal decomposition, thermal
dissociation).
(b) Write correctly the balanced equations for each of the reactions mentioned in the
above statements.
Q.
Define the following terms :
(i) pH-scale (ii) Neutralization.
Q.
(i) Outline the steps that would be necessary to convert insoluble Lead (II) oxide into
insoluble Lead chloride.
(ii) Write the balanced equations for the reaction required to convert insoluble Lead (II)
oxide into insoluble Lead chloride.
(iii) If iron reacts with dilute sulphuric acid, what will be the products of sulphuric acid?
(iv) A solution of Iron (III) chloride has a pH less than 7.Is the solution acidic or alkaline?
Q.
From the following list of substances, choose the one substance in each case which
matches the description (a) to (f) given below :
(Write down the names exactly as they are given in the list. Do not write formulae.)
Ammonium nitrate, Calcium Hydrogen carbonate, Copper Carbonate, Lead carbonate,
Lead nitrate, Potassium nitrate, Sodium carbonate, Sodium Hydrogen carbonate, Zinc
carbonate.
(a) A Hydrogen carbonate which exists in the solid state.
(b) A carbonate not decomposed by heat.
(c) A green coloured Carbonate which turns black on heating.
(d) a nitrate which gives off only Oxygen when heated.
(e) A nitrate which on heating decomposes into Dinitrogen oxide (Nitrous oxide) and
steam.
(f) A nitrate which gives off Oxygen and Nitrogen dioxide when heated.
Q.
Some methods used for the laboratory preparation of salt are
A – Metal + acid
B – Carbonate + acid
C – Precipitation
D – Direct combination
E – Titration
Copy and complete the following table :
Salt
Method of Preparation
mmonium sulphate
Titration
Calcium carbonate
Iron (III) chloride
Lead nitrate
Zinc sulphate
Q.
What do you see when concentrated Sulphuric acid is added to Copper sulphate-5-water.
Q.
Name (formula not acceptable) the gas produced in the following reaction:
Warming Ammonium sulphate solution with Sodium Hydroxide solution.
Q.
State what do you observe when :
(a) Neutral litmus solution is added to an alkaline solution.
(b) Lead nitrate solution and Sodium chloride solution are mixed.
Q.
Copy and complete the table. The table summarizes the observations following the
addition of Barium chloride solution and Lead nitrate solution to solution of Zinc salt. If
nothing happens write no reaction as shown or write white precipitate.
Barium chloride solution
Lead nitrate solution
Zinc chloride
solution
Zinc nitrate
solution
No reaction
Zinc sulphate
solution
Q.
Write the balanced equations for the following reactions:
(a) Dilute hydrochloric and Sodium sulphite.
(b) An acid and an alkali. (Yoy must first write : “The acid is ______ and the alkali is
_______. “ then write the equation)
Q.
Write the terms defined by the following sentences :
(a) A soluble base.
(b) The insoluble solid formed when two solutions are mixed together.
(c) An acidic solution in which there is only partial ionization of the solute molecules.
Q.
Differentiate between the chemical nature of an aqueous solution of Hydrogen chloride
and an aqueous solution of Ammonia.
Q.
Write the balanced equations for the following reactions:
(a) Dilute Nitric acid producing Carbon dioxide.
(b) Dilute Sulphuric acid producing Hydrogen.
(c) Between Lead nitrate solution and dilute Sulphuric acid.
Q.
Choosing substances from the list given below, write equations for the reactions which
you would use in the laboratory to obtain in the box given below the list:
(i) Sodium sulphate (ii) Copper sulphate (iii) Iron (II) sulphate (iv) Zinc carbonate.
Dilute
sulphuric acid
Copper
Copper sulphate
Iron
Sodium carbonate
Sodium
Zinc
Q.
From the formulae listed below, choose one, in each case, corresponding to the salt having
the given description :
AgCl, CuCO3, CuSO4.5H2O, KNO3, NaCl, NaHSO4, Pb(NO3)2, ZnCO3, ZnSO4.7H2O.
(i) An acid salt.
(ii) An insoluble Chloride.
(iii) On treating with concentrated Sulphuric acid, this salt changes from blue to white.
(iv) On heating, this salt changes from green to black.
(v) This salt gives Nitrogen dioxide on heating.
Q.
The following table shows the tests a student performed on two aqueous solutions A, B.
Write down on your answer script the observation (i) and (ii) that were made.
Test
Observation Conclusion
(i) To solution A,
Barium chloride
solution and dilute
Hydrochloric acid
were added.
(i)
A contains
SO4-2 ions
(ii) To solution
B,Silver nitrate
solution and dilute
Nitric acid were
added.
(ii)
B contains
Cl- ions
Q.
The salt which in solution gives a pale green precipitate with NaOH solution and a white
precipitate with BaCl2 solution :
(a) Iron [III] sulphate (b) Iron [II] sulphate (c) Iron [II] chloride (d) Iron [III] chloride.
Q.
State what would you see when Lead nitrate crystals are heated in a dry test-tube?
Q.
How will you convert the followings :
(i) CuSO4 → CuCO3 → CuO → CuSO4
(ii) CuSO4 → Cu(OH)2 → CuO → CuSO4
.
Q.
(i) Define an acid.
(ii) What is an alkali?
(iii) Explain the meaning of the term acid salt.
Q.
Answer the following questions relating to salts and their preparation :
a) What is salt ?
b) What kind of salt is prepared by precipitation ?
c) Name a salt prepared by direct combination. Write the equation for the reaction that
takes place when preparing the salt you have named.
d) What procedure would be used to prepare Sodium salt such as Sodium sulphate. (Give
the name of the procedure only).
Q.
For each of the salts A, B, C and D, suggest a suitable method of preparation which
relates to its description given below :
a) ‘A’ is Sodium salt.
b) ‘B’ is an insoluble salt.
c) ‘C’ is a soluble salt of Copper.
d) ‘D’ is a soluble salt of Zinc.
Q.
(a) Define pH-scale.
(b) The pH value of pure water is 7. Compare the pH values of Sulphur dioxide solution
and Ammonia solution with that of pure water.
Q.
Sulphuric acid can be used to prepare a number of gases in the laboratory. Write
balanced equation for reaction in which the following gases are obtained using dilute
Sulphuric acid as one of the reactants.
(a) Hydrogen (b) Carbon dioxide (c) Sulphur dioxide.
Q.
What is the meaning of the term Water of Crystallization?
Q.
Name :
(i) two bases which are not alkalis.
(ii) a normal salt and acid salt of same acid.
(iii) a salt insoluble in cold water but soluble in hot water.
Q.
From the following list of substances, choose those which meet the description given
below :
Ammonium chloride, Ammonium nitrate, Chlorine, dilute Hydrochloric acid,
Iron, Lead nitrate, Magnesium (IV) oxide, Silver nitrate, Sodium nitrate,
Sulphur. Two compounds whose aqueous solution gives white precipitate with
dilute Hydrochloric acid.
Q.
What do you see when Barium chloride solution is added to dilute Sulphuric acid?
Q.
A solution has a pH of 7. Explain how you would :
(i) increase its pH. (ii) decrease its pH.
Q.
If a solution changes the colour of litmus from red to blue, what can you say about its
pH?
Q.
What can you say about the pH of a solution that liberates Carbon dioxide form Sodium
carbonate?
Q.
Write equations for each of the following reactions:
(i) Chlorine is passed over heated iron.
(ii) Copper sulphate solution is added Sodium hydroxide solution.
Q.
Name from the list of substances given below, the substances you would use to prepare
each of the following salts named in part (a) to (d): Copper, Lead, Sodium, Zinc, Copper
oxide, Lead carbonate, Sodium carbonate solution, dilute Hydrochloric acid, dilute Nitric
acid and dilute Sulphuric acid. (a) Zinc sulphate (b) Copper sulphate (c) Sodium sulphate
(d) Lead sulphate.
Q.
(i) What is the purpose of pH-scale?
(ii) What is the pH of pure water?
(iii) ‘A’ is a soluble acidic oxide, ‘B’ is a soluble base. Compare the pH of pure
water, what will be the pH of :
(1) a solution of ‘A’, (2) a solution of ‘B’.
Q.
Taking Sodium carbonate as an example, give the meaning of the following
terms: (i) Anhydrous (ii) Effloresence.
Q.
Barium chloride solution can be used to distinguish between a Sodium sulphate solution
and a Sodium nitrate solution. How is this done?
Q.
Outline the steps required to convert Hydrogen chloride to anhydrous Iron (III) chloride.
Write the equations for the reactions which take place.
Q.
(i) What are the two steps to change Lead carbonate to Lead chloride?
(ii) Give the name of a soluble salt of lead and write the equation for the action of heat on
this salt.
Q.
Answer the questions below, relating your answer only to the salt in the following list :
Sodium chloride, Anhydrous Calcium chloride, Copper sulphate-5-water.
(a) What name is given to the water in the compound Copper sulphate-5-water?
(b) If Copper sulphate-5-water is heated, the water is driven off, leaving Anhydrou
Copper sulphate. What is the colour of
Anhydrous Copper sulphate?
(c) What is deliquescence?
(d) Which one of the salts in the given list is deliquescent?
Q.
State what you see when :
(a) Silver nitrate solution is added to dilute Hydrochloric acid.
(b) Zinc oxide is heated.
Q.
Write correctly the balanced equations for the following reactions:
(a) Molten Sodium and Chlorine. (b) Iron and dilute Sulphuric acid.
Q.
The compound Na2B4O7.10H2Ois commonly known as Borax. When litmus is added to a
solution of borax, it turns blue. What can you say about the pH of the Borax solution?
Q.
What will you see when Barium chloride solution is added to Iron (II) Sulphate solution?
Q.
How will the action of dilute Hydrochloric acid on Sodium carbonate and Sodium
sulphite enable you to distinguish between these two compounds?
Q.
Write correctly the balanced equations for the reaction of dilute Sulphuric acid with each
of the following: (a) Copper carbonate (b) Lead nitrate solution (c) Zinc hydroxide.
Q.
Solution P has a pH of 13, solution Q has a pH of 6 and solution R has a pH of 2.
(i) Which solution will liberate Ammonia from Ammonium sulphate?
(ii) Which solution is a strong acid?
(iii) Which solution contains solute molecules as well as ions?
Q.
What are the term defined in each case :
(i) A salt containing a metal ion surrounded by other ions or molecules.
(ii) A bse which is soluble in water.