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Chem Solutions Test Review

Total questions: 55

Worksheet time: 19mins

Name
Class
Date
1.
If a solution has the ability to dissolve more salt, it is classified as _______________.
a)
supersaturated
b)
saturated
c)
unsaturated
d)
monosaturated
2.
What will happen to the concentration if more solvent is added to the solution?
a)
the concentration will increase
b)
the concentration will decrease
c)
the concentration will remain the same
3.

A student takes the moles of solute and divides by the liters of solution. What is she solving for?

a)

percent by volume

b)

percent by mass

c)

Molarity

d)

molar mass

4.

A student used this dimensional analysis setup to answer a question. Where did she get 0.100 moles over 1 Liter?

a)

from the atomic masses on the periodic table

b)

This number is always 0.100 no matter the question

c)

from the Molarity (M) given in the problem

d)

from the percent by volume given in the problem

5.
A student uses this dimensional analysis setup to answer a question.  Where did she find the 85 grams that is above 1 mole?
a)
from the atomic masses on the periodic table
b)
you always use 85 grams over 1 mole
c)
it is the number found with "M"
d)
from the balanced chemical equation
6.

Carbon dioxide dissolved in Coke is an example of which solute-solvent combination?

a)

gas-air

b)

liquid-gas

c)

gas-liquid

d)

liquid-air

7.
The "like dissolves like" rule is the reason why water cannot dissolve
a)
salt
b)
sugar
c)
vinegar
d)
oil
8.

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 at a given temperature. heat it up to dissolve the solute, then cool it down.

d)

dissolve a super amount of solvent in it.

9.

After stirring a solution and solid sugar remains on the bottom, the solution is

a)

Supersaturated

b)

Saturated

c)

Unsaturated

d)

Unstable

10.

The solubility of gases tend to __________ when you increase temperature.

a)

Increase

b)

Decrease

c)

Stays the same

d)

Dissolve

11.

Which of the following is NOT a way to increase the rate of dissolving?

a)

Heating

b)

Cooling

c)

Stirring

d)

Crushing the solute

12.

Substances that conduct electricity and dissolve in water are called

a)

Electrolytes

b)

Non-Electrolytes

c)

Sugars

d)

Solvents

13.

Which compound has the highest solubility at 20 degrees Celsius?

a)

HCl

b)

KCl

c)

KI

d)

NaCl

14.

How many grams are needed to saturate HCl at 50 degrees Celsius?

a)

75

b)

58

c)

15

d)

92

15.

At what temperature does the gas, SO2 , have the lowest solubility?

a)

0oC

b)

10oC

c)

40oC

d)

90oC

16.

M1V1=M2V2

a)

Dilution Formula

b)

Molarity formula

c)

percent by mass formula

d)

percent by volume formula

17.

When examining a Solubility curve, the area below the curve is?

a)

unsaturated

b)

saturated

c)

supersaturated

d)

full of Moles

18.

When examining a Solubility curve, the area above the curve is?

a)

unsaturated

b)

saturated

c)

supersaturated

d)

full of Moles

19.

When examining a Solubility curve, the area along the curve is?

a)

unsaturated

b)

saturated

c)

supersaturated

d)

full of Moles

20.

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

a)

NaCl

b)

Cl2

c)

CCl4

d)

C6H6

21.

What happens when you try to mix a polar and a non-polar substance?

a)

They mix evenly

b)

They mix, but unevenly

c)

They don't mix

d)

They always explode

22.
Which types of compounds dissolve easily in water?
a)
Polar and Nonpolar
b)
Polar and Ionic
c)
Nonpolar and Ionic
d)
Covalent and Nonpolar
23.

Oils are ______________ and tend to dissolve other molecules that are __________________.

a)

nonpolar, polar

b)

polar, nonpolar

c)

polar, polar

d)

nonpolar, nonpolar

24.

When ionic compounds dissolve in water, the ions

a)

dissociate and are free to conduct electricity

b)

dissolve and tightly hold on to their electrons

c)

are resistant to electrical impulses

d)

none of these

25.
Which represents the dissociation of 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)
26.
When 2.2 grams of NaCl are poured into a solution of salt, the NaCl dissolves. What can be determined about the original solution from this observation?
a)
the solution was saturated
b)
the solution was hypersaturated
c)
the solution was supersaturated
d)
the solution was unsaturated
27.
A student is testing the rate of dissolution of a whole antacid tablet versus a crushed tablet. The crushed tablet would —
a)
take the same time to dissolve
b)
take more time to dissolve
c)
dissolve slower
d)
dissolve faster
28.

What is the solvent in CaCl2(aq)?

a)
Ca
b)
Cl
c)
there is none
d)
water
29.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
30.
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
31.
When using "like dissolves like", you are looking at what similarity in solvent and solute?
a)
mass
b)
energy
c)
polarity
d)
state of matter
32.
Which salt is LEAST soluble at 0 ºC?
a)
K2Cr2O7
b)
KNO3
c)
 KClO3
d)
Ce2(SO4)3
33.
When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.
a)
concentrated 
b)
Diluted
34.
If an electrical current can run through a solution, it is said to contain
a)
magic
b)
nonelectrolytes
c)
electricity
d)
electrolytes
35.

____________ is the process whereby particles of a solvent completely surround the particles of a solute, disperse them throughout the solvent particles, and hold them in solution.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

36.

Which one of the following should be increased in order to increase the solubility of a gas?

a)

Temperature

b)

Pressure

37.

Compared to pure water, a NaCl solution would have a:

a)

higher boiling point and higher freezing point

b)

lower boiling point and lower freezing point

c)

higher boiling point and lower freezing point

d)

lower boiling point and higher freezing point

38.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
39.

The drawings below represent beakers of aqueous solutions. Each o represents a dissolved solute particles.Which solution is most concentrated?

a)

A

b)

B

c)

C

d)

D

e)

E

40.

The drawings below represent beakers of aqueous solutions. Each o represents a dissolved solute particle.Which solution is least concentrated?

a)

A

b)

B

c)

C

d)

E

e)

F

41.

By adding water to a concentrated solution, you are making it more

a)

Concentrated

b)

Dilute

c)

Acidic

d)

Basic

42.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
43.
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
44.
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
45.

Table salt (NaCl) dissolves into water because...

a)

table salt is ionic and water is ionic

b)

table salt is ionic and water is polar.

c)

table salt is nonpolar and water is nonpolar too.

d)

table salt is ionic and water is nonpolar.

46.
Why will sugar dissolve in water?
a)
sugar is ionic
b)
sugar has a similar polarity to water
c)
sugar will not dissolve in water
d)
sugar has similar energy to water
47.

Which of the following is a heterogeneous mixture

a)

water

b)

salt dissolved in water

c)

Chex mix

d)

air

48.

Which of the following has components in the most uniform arrangement?

a)

Heterogeneous mixture

b)

Colloids

c)

Suspensions

d)

Solutions

49.
The Tyndall effect is used to distinguish between 
a)
gases and solids
b)
solutions and colloids
c)
solvent and suspensions
d)
all of these 
50.
Which of the following will produce crystals if disturbed?
a)
 saturated solutions
b)
colloids
c)
supersaturated solutions
d)
unsaturated solutions
51.

If aqueous solutions of equal Molarity were made from the following ionic compounds, which would be expected to lower the freezing point of water the MOST?

a)

NaCl

b)

BaCl2

c)

MgSO4

d)

AlCl3

52.

Which types of compounds dissolve easily in oil?

a)

Polar and Nonpolar

b)

Polar and Ionic

c)

Nonpolar and Ionic

d)

Covalent and Nonpolar

53.

The red mixture scatters light, therefore, it must be

a)

a solution

b)

a colloid

c)

pure water with food coloring

d)

salt water with food coloring

54.

If lithium bromide dissociated in water, which of its ions would have the largest radius?

a)

lithium

b)

bromide

55.

If sodium chloride dissociated in water, which of its ions would have the largest radius?

a)

sodium

b)

chloride

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