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Solutions Unit

Total questions: 60

Worksheet time: 2hrs 2mins

Name
Class
Date
1.
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
2.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
3.

What is the part of a solution that dissolves?

a)

Solute

b)

Solvent

c)

Solution

d)

Mixture

4.

In the picture, a powder will be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)

agitate or stir the powder in the liquid

b)

freeze the mixture

c)

add more powder to the liquid

d)

store the mixture in a dark place

5.

How many grams of sodium nitrate, NaNO3, are soluble in 100 g of water at 10 ºC?

a)

80 grams

b)

100 grams

c)

40 grams

d)

10 grams

6.
A _______ solution contains more solute than would normally dissolve at a certain temperature.
a)
unsaturated
b)
suspended
c)
saturated
d)
supersaturated
7.

Johnny Boy dissolves the maximum amount of KF in H2O, heats it up and dissolves more, then lets it cool down. The solution is _______________

a)

diluted

b)

unsaturated

c)

saturated

d)

supersaturated

8.

What is the term for when a solid does not dissolve in?

a)

soluble

b)

insolube

c)

immiscible

d)

miscible

9.

Katie is home making sweet tea. She adds sugar and stirs until it dissolve. However, Katie decides to add more sugar. If more sugar was able to dissolve, what can you determine about the original solution?

a)

It was saturated because Katie was able to dissolve more sugar.

b)

It was unsaturated because Katie was able to dissolve more sugar.

c)

It was supersaturated because Katie was able to dissolve more sugar.

10.
What is dissociation?
a)
Breaking the solute into small pieces and spreading throughout the solvent.
b)
The process in which an ionic compound separates into ions in a solution.
c)
The process in which neutral molecules lose or gain electrons
d)
The substance that does the dissolving in a solution.
11.

What is solubility?

a)

the ability of a substance to dissolve.

b)

the ability of a substance to melt.

c)

the ability of a substance to freeze.

d)

the ability of a substance to evaporate.

12.
Which of the following is a non-electrolyte?
a)
CaO
b)
NaOH
c)
BaCl2
d)

NH3

13.

What is solvation?

a)

the process of a solute particle being surrounded by solvent particles.

b)

the process of a solute breaking apart into ions, which are then surrounded by a solvent.

c)

the process of a solvent particle being surrounded by solute particles.

d)

the process of a solvent breaking apart into ions, which are then surrounded by a solute.

14.

A solution that contains the maximum amount of solute dissolved is

a)

an unsaturated solution.

b)

a saturated solution.

c)

a nonsaturated solution.

d)

a supersaturated solution.

15.

Which compound has the highest solubility at 10oC?

a)

SO2

b)

KI

c)

KClO3

d)

NaNO3

16.

Assuming 80 grams of NaNO3 are dissolved at 30oC, what can be said about the solution?

a)

It is a saturated solution

b)

It is a supersaturated solution

c)

15 more grams can be dissolved

d)

The solution is unstable

17.

Calculate the mass of KCl needed to produced 100ml of a .75M KCl solution

a)

5.6g KCl

b)

2.4g KCl

c)

38.7g KCl

d)

.07g KCl

18.

8.3 moles of NaCl are dissolved in 3.4L of solution. Calculate the molarity.

a)

2.4M NaCl

b)

.03M NaCl

c)

8.3M NaCl

d)

18M NaCl

19.

How would you describe NH4NO3

a)

Soluble

b)

Insoluble

c)

Slightly Soluble

d)

Unknown

20.

200ml is equal to what volume in liters?

a)

.2 liters

b)

2 liters

c)

20 liters

d)

.02 liters

21.

4.75 liters is equal to what volume in milliliters?

a)

475 ml

b)

47.5 ml

c)

4,750 ml

d)

47,500 ml

22.

What happens to a supersaturated solution if it is destabilized?

a)

A supersaturated solution can't be destabilized

b)

The solution EXPLODES

c)

The solute precipitates out of solution

d)

The solution will release bubbles

23.

180g C6H12O6 are dissolved in 2000ml of solution. Calculate the concentration.

a)

1M C6H12O6

b)

.5M C6H12O6

c)

2M C6H12O6

d)

.25M C6H12O6

24.

How many moles of KMnO4 are in 0.250 L of a 1.35 M solution?

a)

0.338 moles

b)

540 moles

c)

0.185 moles

d)

1.35 moles

25.

What is the molarity of 6.73 grams of Na2CO3 dissolved in 0.250L of water? Molar mass of Na2CO3 is 106 g.

a)

26.9 M

b)

0.037 M

c)

3.94 M

d)

0.254 M

26.

How can you increase the molarity of a solution?

a)

add solute

b)

add solvent

c)

pour out some of the solution

d)

all of the above

27.

The ratio of the number of moles of solute particles to the volume of solution is the ________ .

a)

mole ratio

b)

molity

c)

molarity

d)

saturation

28.

When 50 grams of potassium chloride, KCl, is dissolved in 100 grams of water at 50 oC, the solution can be correctly described as:

a)

unsaturated

b)

saturated

c)

supersaturated

d)

none of the above

29.

Which solution will be unsaturated when 70 grams is dissolved in 100 g of water at 10 oC?

a)

Ce2(SO4)3

b)

NaNO3

c)

KCl

d)

CaCL2

30.

gHow many grams of undissolved salt are in a beaker containing 80 g of Pb(NO3)2 in 100 g of water at a temperature of 30 oC?

a)

14 g

b)

0

c)

80 g

d)

20 g

31.

Which of the following compounds is soluble in water?

a)

PbBr2

b)

MgCl2

c)

BaSO4

d)

CaCO3

32.

Which of the following compounds is insoluble in water?

a)

(NH4)2S

b)

Na2O

c)

LiOH

d)

Al2O3

33.

Which of the following is an ionic compound that dissociates in water?

a)

NaCl

b)

Cl2

c)

CCl4

d)

C6H6

34.

Which of these solutes is most likely a gas?

a)

NH3

b)

NaNO3

c)

KNO3

d)

NaCl

35.

which is supersaturated at 50 g and 50 degrees Celsius

a)

KClO3

b)
KNO3
c)
NaNO3
d)

NH4ClNH_4Cl  

36.
Graph that shows the amount of solute that can be dissolved in 100 g of water at a certain temperature.
a)
Solubility curve
b)
Saturation curve
c)
Concentration curve
d)
Molarity curve
37.
Solubility refers to the ____ of solute that can dissolve in a certain volume or mass of solvent, at a certain temperature.
a)
Volume
b)
Proportion
c)
Mass
d)
Particles
38.
An ______ is a compound that breaks apart in water, forming charged particles (ions) that can conduct electricity.
a)
electrolyte
b)
nonelectrolyte
c)
polar molecule
d)
non polar molecule
39.
How many more grams of KNO3 dissolve at 50 ⁰C compared to 0 ⁰C?
a)
85 g
b)
15 g
c)
70 g
d)
100 g
40.
How many grams of SO2 can dissolve at 50 ⁰C?
a)
5 g
b)
10 g
c)
20 g
d)
39 g
41.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
42.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

43.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

44.

Which of the following will produce crystals if cooled or disturbed?

a)

unsaturated solution

b)

saturated solution

c)

supersaturated solution

d)

all of the above

45.

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

46.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

47.

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

48.

The term molar, which describes a solution's concentration, is written as?

a)

M

b)

mol

c)

g

d)

g/L

49.

Molarity is ...

a)

grams of solute/deciliters of solvent.

b)

grams of solute/liters of solution.

c)

moles of solute/liters of solution.

d)

moles of solute/milliliters of solvent.

50.
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
51.

What mass in (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid (HBr)?

a)

53.6

b)

1.44

c)

1.23

d)

34.5

52.

How many mL of 0.5M HNO3 would be needed to react with 85mL of 0.75M KOH?

a)

127.5mL

b)

0.1275mL

c)

31.9mL

d)

0.031875mL

53.

To convert liters of a solution to moles, one should:

a)

divide by the molarity

b)

multiply by the molarity

c)

multiply by the molar mass

d)

divide by the molar mass then multiply by the speed of light squared

54.

To convert mL to L, one should:

a)

divide by 1000

b)

multiply by 1000

c)

divide by 100

d)

multiply by 100

55.

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

56.

As water is added to a 0.10 M NaCl aqueous solution, the conductivity of the resulting solution

a)

decreases because the concentration of ions decreases

b)

decreases, but the concentration of ions remains the same

c)

increases because the concentration of ions decreases

d)

increases, but the concentration of ions remains the same

57.

Which of the following solutes will result in a solution with the strongest conductivity?

a)

1.0 M C6H12O6

b)

1.0 M MgBr2

c)

2.0 M NaCl

d)

2.0 M CaF2

58.

Which describes an Electrolyte?

a)

Substance that give out ions when dissolved in water, which are able to conduct electricity

b)

Substances that prehibit electricity from traveling across a solvent

c)

A chemical used to combust flames in a laboratory setting

d)

A type of current that is utilized to determine if there is a blockage anywhere in the system.

59.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

60.
How many grams of solute are dissolved in 125.0 mL 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

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