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Solubility PRACTICE quiz

Total questions: 55

Worksheet time: 1hrs 23mins

Name
Class
Date
1.
At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?
a)
60 ºC
b)
30 ºC
c)
50 ºC
d)
83 ºC
2.
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
3.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
4.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
5.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
6.
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. 
7.
Which solute does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
8.
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
9.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
10.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
11.
When 42 grams of potassium chloride, is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
12.

Which substance's solubility changes the most from 0 degrees Celsius to 100 degrees Celsius?

a)

NH3

b)

NaCl

c)

KI

d)

KNO3

13.

Which substance is most soluble at 20 degrees Celsius?

a)

NH3

b)

HCl

c)

NaNO3

d)

KI

14.

At what temperature (in degrees Celsius) does KNO3 have a solubility of 85 g/100 g H2O?

a)

20

b)

30

c)

40

d)

50

15.

You have a solution of NaNO3 containing 100 grams at 75 degrees Celsius. Your solution is...

a)

saturated

b)

unsaturated

c)

supersaturated

d)

super duper saturated :)

16.

The substance(s) being dissolved is called the ____________

a)

solution

b)

solvent

c)

solute

d)

solvation

17.
In a sample of salt water, NaCl would be considered the ______.
a)
Solution
b)
Solute
c)
Solvent
d)
Solvation
18.

You are making Kool-aid with sugar, Kool-aid powder, and water. What is the solvent?

a)

water

b)

kool-aid powder

c)

sugar

d)

kool-aid powder and sugar

19.

Based on the picture, which of the following will be the solute when the substances are mixed?

a)

The water in the glass

b)

The glass that holds the solution

c)

The solution containing both powder and water

d)

The powder on the spoon

20.

Water is the most common ____.

a)

solute

b)

solvent

c)

solution

d)

mixture

21.

Solutes dissolve quicker in _________ water.

a)

cold

b)

warm

22.

Solutes dissolve quicker if you stir them.

a)

true

b)

false

23.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspension
c)
Colloid
24.

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

25.

Gases are more soluble at ______temperatures and _____pressures.

a)

high, low

b)

low , high

c)

high, high

d)

low, low

26.

If water is a polar molecule, then which of the following must be nonpolar

a)

sugar

b)

salt

c)

oil

d)

vinegar

27.

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

a)

both are polar

b)

both are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

28.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

29.

Molarity is defined as _________ divided by ___________

a)

mol, liters

b)

mol, kg

c)

kg, liters

d)

liters, kg

30.

If a solute dissolves in water than it is_____.

a)

soluble

b)

insoluble

c)

solute

d)

solvent

31.

Label the diagram with the appropriate word to describe changing the state of matter.

a)

condensation

b)

imitation

c)

deposition

d)

freezing

e)

melting

f)

evaporation

g)

sublimation

1
2
3
4
5
6
1)
2)
3)
4)
5)
6)
32.

The ___ does the dissolving, while the ____ gets dissolved.

a)

solvent, solute

b)

solute, solvent

c)

solute, solution

d)

solution, solute

33.

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

34.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

35.

What is the molarity of a solution in which 3.0 moles of NaCl is dissolved in 1.5 L of water

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

36.
Calculate the molarity of the following solution:  1.0 mole of KCl in 750.0 mL of solution.
a)
0.750 M
b)
99 M
c)
1.3 M
d)
2.0 M
37.

What is the molarity of a solution made by adding 1.565 moles of Pb(NO3 )2 to enough water to make 500. mL of soution?

a)

300. M

b)

31.3 M

c)

3.13 M

d)

1.56 M

38.
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
39.

Why doesn't oil dissolve in water?

a)

Oil is polar and water is nonpolar and are not attracted to each other.

b)

Both are polar substances and "likes" repel.

c)

Oil is nonpolar and water is polar and are therefore not attracted to each other.

d)

Both are nonpolar substances and only "opposites" attract.

40.
What is the percent composition of a sugar solution where 10 grams of sugar is added to 100 grams of water?
a)
.10%
b)
0.091%
c)
9.090909%
d)
9.1%
41.
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
42.
What is the percent-by-mass, concentration of sucrose in a solution made by dissolving 7.6 g of sucrose in 83.4 g of water?
a)
0.0835
b)
2.78
c)
8.35
d)
0.0278
43.

What is the concentration of O2(g), in parts per million, in a solution that contains 0.008 gram of O2(g) dissolved in 1000. grams of H2O(l)?

a)

0.8 ppm

b)

80 ppm

c)

8 ppm

d)

800 ppm

44.

A 2400.-gram sample of an aqueous solution contains 0.012 gram of NH3. What is the concentration of NH3 in the solution, expressed as parts per million?

a)

5.0 ppm

b)

15 ppm

c)

20. ppm

d)

50. ppm

45.

The chemist determined that a 175-gram sample of the

town’s water contains 0.000 250 gram of fluoride ions.


How many parts per million of fluoride ions are present in the analyzed sample?

a)

IDK

b)

1.43

46.

Molarity = ​ (a)   of ​ (b)   / ​ (c)   of ​ (d)  

Choose from the below words
solution
liters
solute
moles
grams
solvent
molar mass
molarity
47.

determine the molarity of 10.5kg of Na2SO4 in 19.95L of solution.

48.

What volume is needed to make a 2.45 M solution of KCl using 0.50 mol of KCl?

a)

4.9 L

b)

0.20 L

c)

1.2 L

49.

Organize these sweet tea concentrations from least sweet (1) to most sweet (2)

a)

.02 M

b)

.50 M

c)

1.0 M

d)

1.5 M

e)

2.0 M

1)
2)
3)
4)
5)
50.

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

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

51.
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
52.
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
53.

Which one of the following diagrams has the highest boiling point?

a)

1

b)

2

c)

3

d)

4

e)

5

54.

Which solution below has the highest boiling point?

a)

NaCl 1 M

b)

CaCl2 1 M

c)

C6H12O6 1 M

d)

AlCl3 1 M

55.

The freezing point of water is...

a)

100oC

b)

0oC

c)

-10oC

d)

150oC

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