BCLN CHEMISTRY 11 - Rev. July/2014
Unit 6 ~ Learning Guide Name: ______________________________
Instructions:
Using a pencil, complete the following notes as you work through the related lessons. Show ALL
work as is explained in the lessons. You are required to have this package completed BEFORE
you write your unit test. Do your best and ask questions if you don’t understand anything!
Mixtures and Solutions:
1. In the table below list 3 differences between pure substances and mixtures
Pure Substances
Mixtures
Has constant physical properties
Has variable physical properties
Has constant chemical properties
Has variable chemical properties
Are homogeneous and so exhibit one phase
May be homogenous or heterogeneous with
multiple phases
Students may list other possibilities
2. A solid dissolved in a liquid is known as an amalgam while a solid dissolved in another solid is
known as what?
An alloy
3. What are four factors that affect solubility?
Molecular polarity, size of molecules, temperature, pressure
Molar concentration:
1. Write the long form and the short form of the concentration formula
=
Page 1 of 10
C=
BCLN CHEMISTRY 11 - Rev. July/2014
2. If 1.60 mol of table sugar (C12H22O11) is dissolved to give 750. mL of solution, what is the molar
concentration of the solution?
=
=
.
.
= . 3. A solution of epsom salts may be prepared by dissolving 35.6 g of magnesium sulfate in
sufficient water to make 500.0 mL of solution. Determine the molar concentration of the epsom
salts solution.
Magnesium Sulfate = MgSO4
Molar Mass = 1 Mg + 1 S + 4 O = 1(24.31) + 1(32.06) + 4(16.00) = 120.37 g/mol
.
!
=
=
. " .
.
= . " = . " 4. Hydrogen peroxide, H2O2, forms a colorless solution. How many moles of H2O2 are found in
3.50 L of disinfectant solution that has a concentration of 0.450 M H2O2?
=
×$= .
!
.
= 1.58 mol %
5. What mass of nitre, KNO3•8H2O, is necessary to make 400. mL of a 0.0500 mol/L solution?
Molar Mass Nitre = 1 K + 1 N + 11 O + 16 H = 1(39.10) + 1(14.01) + 11(16.00) + 16(1.01)
Molar Mass Nitre = 245.27 g/mol
.
&'
= . " &'
•(%
!
.
&'
&'
•(%
•(%
Page 2 of 10
•(%
!
.
&'
&'
•(%
•(%
BCLN CHEMISTRY 11 - Rev. July/2014
6. Salt of lemon is a dilute solution of potassium binoxalate (KHC2O4•H2O) often used to remove
ink stains. What volume of 1.25 M salt of lemon contains 6.00 mol of potassium binoxalate?
)=
$
=
.
.
/
= .
7. Commonly called bleach, sodium hypochlorite (NaOCl) has many uses as a strong base and
cleaner. What volume (in mL) of 1.70 M NaOCl can be prepared from 54.7 g of solute?
Molar Mass NaOCl = 1 Na + 1 O + 1 Cl = 1(22.99) + 1(16.00) + 1(35.45) = 74.44 g/mol
. '
$ !
.
'
$
'
$
!
'
.
$
'
$
= .
Polarity in Molecules:
1. What is the definition of electronegativity?
The attraction that an atom has for a covalently bonded electron pair
2. Why is CCl4 not a polar molecule?
It is a symmetrical molecule which means all polar bonds cancel each other out
3. Fill in the following table. It is vital that you have this information memorized for your test!
Solute
dissolves in
Solvent
Non-polar
dissolves in
non-polar
Polar
dissolves in
polar
Ionic
dissolves in
polar
Page 3 of 10
BCLN CHEMISTRY 11 - Rev. July/2014
Dissociation and Ionic Equations:
1. Why do covalent (molecular) dissolve but not dissociate?
They are made of whole neutral molecules not ions.
2. For each of the following write i) a balanced chemical formula equation, ii) a total ionic equation
and iii) a net ionic equation. Remember if you are given the name of an ionic compound you
must balance the formula correctly!
a) Magnesium metal is placed in a solution of hydrochloric acid and reacts to form a magnesium
chloride solution and hydrogen gas
i)
Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
ii)
Mg(s) + 2 H+(aq) + 2 Cl-(aq) → Mg2+(aq) + 2 Cl-(aq) + H2(g)
iii)
Mg(s) + 2 H+(aq) → Mg2+(aq) + H2(g)
b) Zinc metal is placed in a silver nitrate solution and reacts to form silver metal and a zinc nitrate
solution.
i)
Zn(s) + 2AgNO3(aq) → 2Ag(s) + Zn(NO3)2(aq)
ii)
Zn(s) + 2Ag+(aq) + 2NO3- (aq) → 2Ag(s) + Zn2+(aq) + 2NO3-(aq)
iii)
Zn(s) + 2Ag+(aq) → 2Ag(s) + Zn2+(aq)
c) Barium chloride solution is added to lead(II) nitrate solution in a double replacement reaction.
One lead containing precipitate forms while the other product remains in solution.
i)
BaCl2(aq) + Pb(NO3)2(aq) → PbCl2(s) + Ba(NO3)2(aq)
ii)
Ba2+(aq)+2Cl-(aq)+Pb2+(aq)+2NO3-(aq) → PbCl2(s)+Ba2+(aq)+2NO3-(aq)
iii)
2Cl-(aq) + Pb2+(aq) → PbCl2(s)
Page 4 of 10
BCLN CHEMISTRY 11 - Rev. July/2014
d) Sulfuric acid is added to sodium hydroxide. No precipitate forms from this neutralization
reaction.
i)
H2SO4(aq) + 2NaOH(aq) → 2H2O(l) + Na2SO4(aq)
ii)
2H+(aq) + SO42-(aq) + 2Na+(aq) + 2OH-(aq) → 2H2O(l) + 2Na+(aq) + SO42-(aq)
iii)
H+(aq) + OH-(aq) → H2O(l)
e) Aqueous chlorine is added to a solution of aluminum bromide in a single replacement reaction
which forms no precipitate and bromine liquid.
i)
3 Cl2(aq) + 2 AlBr3(aq) → 2 AlCl3(aq) + 3 Br2(l)
ii)
3Cl2(aq) + 2Al3+(aq) + 6Br-(aq) → 2Al3+(aq) + 6Cl-(aq) + 3Br2(l)
iii)
Cl2(aq) + 2Br-(aq) → 2Cl-(aq) + Br2(l)
3. What is the concentration of each ion in a 5.50 M solution of aluminum sulfate? Write a
dissociation equation and put the correct concentration below each ion.
Dissociation equation: Al2(SO4)3(aq) → 2 Al3+(aq) + 3 SO42-(aq)
Concentration:
5.5 M
Page 5 of 10
11.0 M
16.5 M
BCLN CHEMISTRY 11 - Rev. July/2014
4. What is the concentration of each ion formed when 94.5g of nickel (III) sulphate is dissolved into
850.0 mL of water? You will first need to calculate the concentration of the chemical then write a
dissociation equation and put the correct concentration below each ion.
Molar Mass Ni2(SO4)3 = 2 Ni + 3 S + 12 O = 2(58.69) + 3(32.06) + 12(16.00) = 405.56 g/mol
" .
' (
=
=
.
) !
.(
' (
.
' (
= .
)
= .
)
' (
' (
)
)
Dissociation equation: Ni2(SO4)3(aq) → 2 Ni3+(aq) + 3 SO42-(aq)
Concentration:
0.274 M
0.548 M
0.822 M
5. A 0.657 g sample of sodium hydroxide and a 1.62 g sample of strontium hydroxide are dissolved
in 100. mL of solution. Assuming that no reaction occurs, calculate the concentration of each ion
in the solution.
Molar Mass NaOH = 1 Na + 1 O + 1 H = 22.99 + 16.00 + 1.01 = 40.00 g/mol
Molar Mass Sr(OH)2 = 1 Sr + 2 O + 2 H = 1(87.62) + 2(16.00) + 2(1.01) = 121.64 g/mol
'
%= .
( %) = .
'
% ×
( %) ×
'
.
'
.
%
%
( %)
( %)
= .
= .
mols Na+ = mols NaOH = 0.0164 mol
=
=
.
.
mols Sr2+ = mols
=
=
.
.
= .
( %)
= .
'
.
( -)
= 0.0133 mol
.
( -)
mols OH– = (1 × mols NaOH) + (2 × mols Sr(OH)2)
= 0.0164 mol + (2 x 0.0133) mol = 0.0430 mol OH–
=
=
.
.
= .
%(/ -)
Page 6 of 10
'
( %)
%
BCLN CHEMISTRY 11 - Rev. July/2014
Electrolytes:
1. Why are covalent solutions unable to conduct electricity?
They do not form ions
2. Name 3 common non-electrolytes
Sugar, ethanol and ethylene glycol. Other answers are possible
3. Fill in the following table
Ion Charge
Ion Name
Positive
Cation
Negative
Anion
4. Why does not much current flow through a weak electrolyte solution?
Because most of the compound stays in molecular form meaning there are not many ions
5. How can you create an electrolyte other than dissolving a compound?
Melt an ionic compound
Page 7 of 10
BCLN CHEMISTRY 11 - Rev. July/2014
Chemical Reactions and Solutions:
1. Use the reaction below to answer the following questions. Remember that M = mol/L
K2CO3(s) + 2HCl(aq) → 2KCl(aq) + H2O(l) + CO2(g)
a) What volume in mL of 3.00 M hydrochloric acid is required to completely react with 20.0 g of
potassium carbonate?
Molar Mass K2CO3 = 2 K + 1 C + 3 O = 2(39.10) + 12.01 + 3(16.00) = 138.21 g/mol
. & $
×
& $
(.
& $
×
%$
×
& $
%$
.
%$
= 0.0965 L
= 96.5 mL HCl
b) Determine the number of litres of carbon dioxide gas that can be created at STP when 300. mL
of 3.00 M hydrochloric acid reacts completely.
.
.
%$ × %$
×
%$
$
%$
×
. $
=
$
. $
c) What volume in mL of 0.250 M hydrochloric acid is required to produce 8.00 g of water?
Molar Mass H2O = 2 H + 1 O = 2(1.01) + 16.00 = 18.02 g/mol
(.
%
×
%
(.
%
×
%$
%
×
%$
.
%$
= 3.55 L HCl
= 3550 mL HCl
d) What mass of potassium carbonate is needed to completely react with 375 mL of 1.65 M
hydrochloric acid?
.
%$ × .
%$
%$
×
& $
%$
Page 8 of 10
×
(.
& $
& $
=
. ( & $
BCLN CHEMISTRY 11 - Rev. July/2014
2. What is the molar concentration of each ion if 153.7g of tantalum (V) phosphate are dissolved in
350. mL of solution?
Molar Mass Ta3(PO4)5 = 3 Ta + 5 P + 20 O = 3(180.95) + 5(30.97) + 20(16.00) = 1017.70 g/mol
.
=
0
=
(1
) !
= .
.
.
0
.
(1
0
)
(1
0
)
= .
(1
0
(1
)
)
Dissociation equation: Ta3(PO4)5(aq) → 3 Ta5+(aq) + 5 PO43-(aq)
Concentration:
0.431M
1.29 M
2.16 M
3. What is the concentration of each ion in solution when 97.7 grams of Be3P2 and 121 grams of
(NH4)3P are dissolved to make 500. mL of solution?
Molar Mass Be3P2 = 3 Be + 2 P = 3(9.01) + 2(30.97) = 88.97 g/mol
Molar Mass (NH4)3P = 3 N + 12 H + 1 P = 3(14.01) + 12(1.01) + 1(30.97) = 85.12 g/mol
1 =" .
2
2
('% ) 1 =
= .
=
2
1
((."
2
1
('% ) 1!
= .
('% ) 1
( .
('% ) 1
2
('% ) 1
mols Be2+ = 3 x mols 2
=
1 !
.
.
= .
1 = 3(1.10) = 3.30 mol
2
.
( -)
mols NH4+ = 3 x mols (NH4)3P = 3(1.42) = 4.26 mol
=
=
.
.
= (.
'% .(
-)
mols P3- = 2 x mols Be3P2 + mols (NH4)3P = 2(1.10) + 1.42
= 3.62 mol P3=
=
.
.
= .
1( /-)
Page 9 of 10
1
BCLN CHEMISTRY 11 - Rev. July/2014
4. What is the molar concentration of each ion when 250. mL of 0.500 M NH4F (aq) are added to
750. mL of 0.600 M (NH4)2CrO4 (aq) ?
Dilutions
3NH6 F8 = .
!
3(NH6 )9 CrO6 8 = .
= .
!
= .
Dissociation equation: NH4F(aq) → NH4+(aq) + F-(aq)
Concentration:
0.125 M
0.125 M
0.125 M
Dissociation equation: (NH4)2CrO4(aq)→ 2NH4+(aq) + CrO42-(aq)
Concentration:
0.450 M
0.900 M
0.450 M
[NH4+] = 0.125 M + 0.900 M = 1.025 M
[F-] = 0.125 M
[CrO42-] = 0.450 M
Answers:
Molar Concentration:
2. 2.1 M
3. 0.592 M MgSO4
6. 4.80 L
7. 432 mL
4. 1.58 mol H2O2
5. 4.91g nitre
Dissociation and Ionic Equations:
3. 11.0 M Al3+(aq) and 16.5 M SO42-(aq)
5. 0.164 M Na+(aq),
4. 0.548 M Ni3+(aq) and 0.822 M SO42-(aq)
0.133 M Sr2+(aq) and
0.430 M OH–(aq)
Chemical Reactions and Solutions:
1. a) 96.5 mL HCl
b) 10.1 L CO2 c) 3550 mL HCl
2. 1.29 M Ta5+(aq) and 2.16 M PO43-(aq)
3. 6.60 M Be2+(aq),
8.52 M NH4+(aq) and 7.24 M P3-(aq)
4. 1.025 M NH4+(aq), 0.125 M F-(aq), and 0.450 M CrO42-(aq)
Page 10 of 10
d) 42.8 g K2CO3