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SBVC Chem 101 Ch 13 Quiz

Total questions: 52

Worksheet time: 4hrs 55mins

Name
Class
Date
1.
How does a solution become supersaturated?
a)
dissolve lots of solute in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a solvent in it. 
2.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Mixture
d)
Homogeneous solution
3.
Describe a solute.
a)
part of solution present in largest amount
b)
gets dissolved
c)
water
d)
surrounds and breaks apart
4.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspensions
c)
Heterogeneous Mixtures
d)
Pure Substances
5.
When a solvent contains as much of the solute as it can hold, the solution is said to be
a)
supersaturated
b)
diluted
c)
saturated
d)
unsaturated
6.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
7.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
8.
What is able to dissolve other substances?
a)
Solute
b)
Salt
c)
Suspension
d)
Solvent
9.
If I dissolve sugar in water, what is the solute?
a)
Water
b)
Hydrogen
c)
Sugar
d)
Carbon
10.
If I dissolve carbon dioxide in water, what is my solvent?
a)
Carbon Dioxide
b)
There is no solvent
c)
Oxygen
d)
Water
11.

The substance being dissolved is called the ________

a)

solvent

b)

solid

c)

solute

d)

solvate

12.

The process of dissolving a substance in solution

a)

solvotion

b)

salvation

c)

solvation

d)

salvution

13.

A non-electrolyte is composed of __________in solution

a)

molecules

b)

molecules and ions

c)

ions

d)

none of the above

14.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

15.

When no more solute dissolves the solution is _________

a)

supersaturated

b)

unsaturated

c)

saturated

d)

supercalifragilisticexpialidocious

16.

Gases are more soluble at ______temps and _____pressures

a)

high, low

b)

low , high

c)

high, high

d)

low, low

17.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

18.

Molarity is defined as _________ divided by ___________

a)

mol, liters

b)

mol, kg

c)

kg, liters

d)

liters, kg

19.

How many mols of HCl are in 3 liters of 2.0M HCl solution?

a)

2.0

b)

1.5

c)

6.0

d)

0.66

20.

A solution is prepared by dissolving 1.29 g of of calcium sulfite 7.3 L of H2O. What is the concentration in percent by mass?

a)

.17%

b)

.017%

c)

5.1%

d)

.0092

21.

A solution is prepared by dissolving 193.6 g of magnesium chlorite in 0.917 L of H2O. What is the concentration in percent by mass?

a)

17%

b)

.017%

c)

5.1%

d)

.0092

22.

A solution is prepared by dissolving 0.0816 g of sodium chloride in 0.883 L of H2O. What is the concentration in percent by mass?

a)

.17%

b)

.017%

c)

5.1%

d)

.0092%

23.

A solution of is prepared by dissolving 810 g of hydrogen chloride in 15.07 L of H2O. What is the concentration in percent by mass

a)

.17%

b)

.017%

c)

5.1%

d)

.0092%

24.

What mass of rubidium sulfide must be added to 7.45 L of H2O to make a solution which is 0.39% by mass?

a)

.17 kg

b)

.017 kg

c)

.029 kg

d)

14 kg

25.

What is the percent by mass of a solution made by dissolving 20.0 g of NaCl into 180.0 g of water?

a)

10.0 %

b)

11.1 %

c)

80.0 %

d)

20.0 %

26.

What mass of water should be added to 22.0 g of KCl to make 5.50% by mass solution?

a)

400 g

b)

40 g

c)

0.25 g

d)

25 g

27.

What is the percent concentration of sugar in pink lemonade if 28 g of sugar is added to 209 g of water?

a)

14.7 %

b)

5.14 %

c)

13.4 %

d)

8.47 %

e)

11.8 %

28.

How many grams of NaNO3 are needed to prepare 100 g of 15.0 % by mass NaNO3 solution? (MM = 85 g/mol)

a)

15 g

b)

1275 g

c)

12.75 g

d)

150 g

29.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
30.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
31.

What is the molarity of 0.068 mol of NaCl in 3.8 L of solution?

a)

0.018 M

b)

0.0011 M

c)

1.052 M

d)

0.062 M

32.

How many grams of solute are dissolved in 0.125 L of 5.00 M NaCl (MM = 58.45)?

a)

0.625 g NaCl

b)

625 g NaCl

c)

36.5 g NaCl

d)

0.04 mol NaCl

33.

Calculate the molarity of the following solution: 1.0 mole of KCl in 0.750 L of solution.

a)

0.750 M

b)

99 M

c)

1.3 M

d)

2.0 M

34.

What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 0.5 L?

a)

300. M

b)

31.3 M

c)

3.13 M

d)

1.56 M

35.
How many moles are needed to make 2.5 L of a 3.8 M solution? 
a)
9.5 mol
b)
0.66 mol
c)
1.5 mol
d)
15 mol
36.

As you put in more solute in the solution, the concentration of the solution will...

a)

increase

b)

decrease

c)

stay the same

37.

As you remove solvent (evaporate the water) from the solution, the concentration (M) will...

a)

increase

b)

decrease

c)

stay the same

38.

What would be the final volume of a solution if you dissolved 2.5 mol of solute to make 7.5 M solution?

a)

0.33 Liter

b)

18.75 Liter

c)

3 Liter

39.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
40.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
41.
How many grams of AgNO3 (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water? 
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
42.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
43.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
44.
What volume of 1.50 M KBr can be made from 15.6 mL of concentrated KBr with a molarity of 9.65 M?
a)
150. mL
b)
151 mL
c)
1.00 L
d)
100. mL
45.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
46.
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
47.

If the temperature stays the same, the solubility of gases in liquids

a)

increases with increasing pressure

b)

cannot reach equilibrium

c)

decreases with increasing pressure

d)

does not depend on pressure

48.

Calcium carbonate reacts with aqueous hydrochloric acid to form calcium chloride solution, water, and carbon dioxide gas in the following equation: CaCO3 (s) + 2 HCl --> CaCl2 (aq) + H2O (l) + CO2 (g) What volume (in mL) of 1.35 M HCl will be needed to completely react with 3.82 g of solid CaCO3?

a)

56.5 mL

b)

47.2 mL

c)

61.6 mL

d)

34.7 mL

e)

124 mL

49.

Aqueous solutions of sodium chloride and lead (II) nitrate react to form solid lead(II) chloride in the following balanced equation: 2 NaCl (aq) + Pb(NO3)2 (aq) --> PbCl2 (s) + 2 NaNO3 (aq) What is the theoretical yield of lead(II) chloride if 250.0 mL of 1.75 M sodium chloride reacts with excess lead(II) nitrate?

a)

78.5 g

b)

93.1 g

c)

45.5 g

d)

60.8 g

e)

59.4 g

50.

Solid iron (II) sulfide reacts with hydrochloric acid to form hydrogen sulfide gas and aqueous iron (II) chloride:

FeS (s) + 2 HCl (aq) --> H2S (g) + FeCl2 (aq) If 145 mL of HCl is needed to completely react with 25 g of iron (II) sulfide, what is the concentration of the HCl solution?

a)

3.1 M

b)

0.68 M

c)

2.7 M

d)

9.0M

e)

3.9 M

51.

Lithium metal reacts with phosphoric acid to form hydrogen gas in the following (dangerous) reaction:

6 Li (s) + 2 H3PO4 (aq) --> 3 H2 (g) + 2 Li3PO4 (aq) What volume of 2.30 M phosphoric acid will be needed to form 19.7 L of hydrogen gas at STP? (Remember: 1 mole of any gas at STP is 22.4 L)

a)

466 mL

b)

255 mL

c)

133 mL

d)

322 mL

e)

75 mL

52.

Solutions of acetic acid and sodium bicarbonate react to form sodium acetate, water and carbon dioxide gas:

HC2H3O2 (aq) + NaHCO3(aq) --> NaC2H3O2 (aq) + H2O (l) CO2 (g) What mass of water will be formed if 145.0 mL of 1.5 M acetic acid is mixed with 195.0 mL of 1.25 M sodium bicarbonate solution? (Note: this is a limiting reactant problem—use a BCA table)

a)

6.7 g

b)

2.5 g

c)

3.9 g

d)

1.6 g

e)

10.4 g

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