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Accel Chem PC #07 NIE and Colligative Properties

Total questions: 49

Worksheet time: 3hrs 51mins

Name
Class
Date
1.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
2.
Molality is measured in
a)
mols per kg
b)
mols per L
c)
mols per kJ
d)
mols per mL
3.
Which technique could increase or speed up the rate of dissolving?
a)
Allowing the mixture to settle
b)
Stirring the mixture
c)
Adding more powder
d)
Adding more water
4.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
5.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
6.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
7.
What is the freezing point of a 1.5 m solution of sucrose in water? (Kf = 1.86°C/m)
a)
-2.8°C
b)
-1.2°C
c)
-0.81°C
d)
0.81°C
8.
Colligative properties depend on the _________ of the solute but not the __________ of the solute.
a)
 concentration; identity
b)
identity; concentration
c)
reactivity; nature
d)
nature; reactivity
9.
A solution has 10 moles of ammonia in 2L of solution. What is the molarity? 
a)
5.0 M
b)
20 M
c)
0.5 M
d)
0.2 M
10.
How many moles of HNO3 are needed to prepare 5L of a 2M solution? 
a)
10 mol
b)
2.5 mol
c)
0.4 mol 
d)
100 mol 
11.
What is the boiling point of a solution if 5.76 mol NaF is dissolved in 3.62 kg of water? (Kb=0.512*C/m)
a)
0.81*C
b)
101.62*C
c)
100.81*C
d)
103.1*C
12.
What is the dissociation factor (i.e. van't Hoff factor) for the compound CH3OH?
a)
1
b)
3
c)
6
d)
9
13.
What is the dissociation factor (i.e. van't Hoff factor) for the compound Na2SO4?
a)
1
b)
3
c)
5
d)
7
14.
Zinc Carbonate (ZnCO3)
a)
Soluble 
b)
Insoluble 
15.
Potassium hydroxide (KOH)
a)
Soluble 
b)
Insoluble
16.
Zinc Hydroxide (Zn(OH)2)
a)
Soluble 
b)
Insoluble
17.
Sodium acetate (NaC2H3O2)
a)
soluble
b)
insoluble
18.

Iron (II) sulfide, FeS, is _______ in water.

a)

soluble

b)

insoluble

19.

What of these is always soluble?

a)

Nitrates

b)

Phosphates

c)

Carbonates

d)

Hydroxides

20.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)

Ca2+(aq) +  2Cl- (aq) → CaCl(s)

b)

Ag+(aq)  +  Cl- (aq) → AgCl(s)

c)

Ag +  Cl  →  AgCl

d)

Ag+  +  Ca2+   →Ag2Ca (s)

21.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
22.
Which of these results in the formation of a precipitate?
a)
AgNO3(aq)  +  NaOH(aq)→
b)
BaNO3(aq)  +  CaCl2(aq)→
c)
NaNO3(aq)  +  KOH(aq)→
d)
More than one of these form precipitates
23.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
24.

What is the result of the reaction between potassium bromide, KBr, and ammonium sulfide, NH4S?

a)

potassium sulfide precipitates

b)

ammonium bromide precipitates

c)

potassium ammonium precipitates

d)

no precipitate is formed

25.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
26.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)

Combination/Synthesis

b)
Decomposition
c)

Single Displacement

d)

Double Displacement

27.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)

Combination/Synthesis

b)
Decomposition
c)

Single Displacement

d)

Double Displacement

28.

Strong electrolytes are good conductors of electricity

a)

True

b)

False

29.

Non-electrolytes do not conduct electricity

a)

True

b)

False

30.

Weak electrolytes are weak conductors of electricity

a)

True

b)

False

31.

Which of the following is generally true?

a)

Polar substances dissolve polar substances

b)

Nonpolar substances dissolve polar substances

c)

Polar substances dissolve nonpolar substances

d)

None of the above

32.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
AgClO3
a)
AgClO3(s) --> Ag(aq) + ClO3(aq) 
b)
AgClO3(s) -->Ag+(aq) + Cl2 (aq) + O2(aq)
c)
AgClO3(s) -->Ag+(aq) + Cl-(aq) + 3O2-(aq)
d)
AgClO3(s) --> Ag+(aq) + ClO3-(aq) 
33.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
NaCl
a)
NaCl  --> Na+ + Cl-
b)
NaCl(s)  --> Na+(aq) + Cl-(aq)
c)
NaCl  --> Na + Cl
d)
NaCl(s) --> Na(aq) + Cl(aq)
34.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
NaOH
a)
NaOH(s) --> Na+(aq) + OH-(aq) 
b)
NaOH --> Na+ + OH- 
c)
NaOH --> Na + OH
d)
NaOH(s) --> NaO-(aq) + H+(aq) 
35.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
LiOH
a)
LiOH(aq) --> Li+(s) + OH-(s) 
b)
LiOH(s) --> Li+ (aq) + OH- (aq) 
c)
LiOH(s) --> Li+(aq) + O2(aq) + H2(aq) 
d)
LiOH(s) --> Li+(aq) + O22-(aq) + H2+(aq) 
36.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
KMnO4
a)
KMnO4(s) --> K+(aq)+ Mn4+(aq) + O4 -(aq)
b)
KMnO4 --> K++ MnO4 - 
c)
KMnO4(s) --> K+(aq) + MnO4 -(aq)  
d)
KMnO4 --> K++ Mn4+ + O4 -
37.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
PbCrO4
a)
PbCrO4(s) ↔ Pb2+(aq) + CrO44-(aq)
b)
PbCrO4(s) ↔ Pb2+(aq) + CrO42-(aq)
c)
PbCrO4(s) ↔ Pb+(aq) + CrO4-(aq)
d)
PbCrO4(s) ↔ Pb4+(aq) + CrO44-(aq)
38.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
ZnCl2
a)
ZnCl2(s) --> Zn2+(aq) + Cl-(aq)
b)
ZnCl2(s) --> Zn+(aq) + 2Cl-(aq)
c)
ZnCl2(s) --> Zn2+(aq) + 2Cl-(aq)
d)
ZnCl2(s) --> Zn+(aq) + Cl-(aq)
39.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
Ca(NO3)2
a)
Ca(NO3)2(s) -->Ca+(aq) + 2NO3- (aq) 
b)
Ca(NO3)2(s) -->Ca2+(aq) + 2NO3- (aq) 
c)
Ca(NO3)2(s) -->Ca2+(aq) + NO3- (aq) 
d)
Ca(NO3)2 -->Ca+ + 2NO3- 
40.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)

1.17 gram

b)
62.7 mol
c)
1.07 mol
d)
62.7 grams
41.

What is the molarity of 4 grams of KNO3 in 3.8 L of solution?

a)

0.01 M

b)

0.02 M

c)

1.05 M

d)

1.08 M

42.

How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?

a)

7.5 mL

b)

15 mL

c)

1333 mL

d)

200 mL

43.

How many moles of solute are present in 50.0 mL of 0.20M KNO3?

a)

10.0 moles solute

b)

0.05 moles solute

c)

1.00 moles solute

d)

0.01 moles solute

44.

Since "like dissolves like", water and oil will not mix because

a)

both of them are polar

b)

both of them are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

45.

When CH3OH is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

3

c)

4

d)

5

e)

6

46.

When KCl (potassium chloride) is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

6

47.

At the same concentration, which salt will have the largest effect on the freezing point?

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

48.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
49.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than

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