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Unit 11: Solutions

Total questions: 41

Worksheet time: 3hrs 59mins

Name
Class
Date
1.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
2.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
3.
How does a solution become supersaturated?
a)
dissolve lots of solvent in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
4.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
5.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
6.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
7.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
8.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
9.
State whether the following compound is soluble or insoluble. potassiun bromide KBr
a)
Soluble
b)
Insoluble
10.
State whether the following compound is soluble or insoluble.  calcium carbonate CaCO3 
a)
soluble
b)
insoluble
11.
State whether the following compound is soluble or insoluble. potassiun bromide KBr
a)
Soluble
b)
Insoluble
12.
State whether the following compound is soluble or insoluble. iron(ii) sulfide FeS
a)
soluble
b)
insoluble
13.
State whether the following compound is soluble or insoluble. Zinc  carbonate ZnCO3 
a)
Soluble 
b)
Insoluble 
14.
State whether the following compound is soluble or insoluble.Silver acetate AgC2H3O2
a)
Soluble 
b)
Insoluble
15.
State whether the following compound is soluble or insoluble.nickel chloride NiCl2
a)
Soluble 
b)
Insoluble
16.
State whether the following compound is soluble or insoluble.sodium nitrate NaNO3
a)
soluble
b)
insoluble
17.
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) →
18.
What is the formula for molarity?
a)
moles/grams
b)
moles/kilograms
c)
moles/milliliters
d)
moles/liters
19.
What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?
a)
2.4 M
b)
0.86 M
c)
1.7 M
d)
0.54 M
20.

Calculate the grams of NaOH present in 10.0 mL of a 2.0 M NaOH solution.

a)

0.8 grams

b)

2000 grams

c)

0.3 grams

d)

5 grams

21.

A 0.500 M solution of NaOH, which contains 0.750 mole of solute, would have a volume, in milliliters

a)

0.667 mL

b)

1200 mL

c)

1500 mL

d)

2100 mL

22.

Calculate the volume of a 5M solution that contains 10 moles of NaOH

a)

0.5 L

b)

1 L

c)

2 L

d)

4 L

23.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
24.
What mass of solute is needed to make 75.0 g of a 3.4% solution?
a)
2.55 g
b)
22 g
c)
0.05 g
25.

What is the concentration of a solution in parts per million if 0.02 grams of NaCl is dissolved in 1000 grams of water?

a)

2 ppm

b)

20 ppm

c)

200 pm

d)

0.2 ppm

26.

What is the concentration of solution (in ppm) made up of 0.005 grams of solute in 350 grams of solution?

a)

14.3 ppm

b)

12.1 ppm

c)

1.4 ppm

d)

9.8 ppm

27.

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

28.
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
29.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
30.
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
31.
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
32.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)
1.07 gram
b)
62.7 mol
c)
1.07 mol
d)
62.7 grams
33.
True or false? Insoluble means that two substances can dissolve in one another.
a)
true
b)
false
34.
What is the molarity of a solution made from 325.4g of AlCl3 with enough water to make 500.0 mL?
a)
4.88 g
b)
4.88 M
c)
2.440 M
d)
2.44 M
35.
How many grams of AgNO3 are needed to prepare 0.125M solution in 250 mL of water? (the molar mass is 169.87g=1 mole)
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
36.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

37.
Liquids with weak intermolecular forces
a)
contain a lot of kinetic energy
b)
easily evaporate
c)
cannot diffuse
d)
freeze easily
38.

According to the reference table, what is the boiling point of ethanoic acid at 80 kPa?

a)

28 oC

b)

100oC

c)

111oC

d)

125oC

39.

At which temperature is the vapor pressure of ethanol equal to the vapor pressure of propanone at 35oC?

a)

35oC

b)

60oC

c)

82oC

d)

95oC

40.
When you increase your altitude, the air pressure 
a)
increases
b)
decreases
c)
stays the same
41.

Which compound has the lowest vapor pressure at 50C?

a)

propanone

b)

ethanoic acid

c)

water

d)

ethanol

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