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Unit 6 - Solubility Practice

Total questions: 40

Worksheet time: 2hrs 0mins

Name
Class
Date
1.

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

2.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
3.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
4.

How many grams of CaCl2, are soluble in 100 g of water at approximately 17 ºC?

a)

58 grams

b)

70 grams

c)

0 grams

d)

12 grams

5.

In a solution, the part that DOES the dissolving-

a)

Strainer

b)

Solvent

c)

Solute

d)

Magnetism

6.

The substance which dissolved in the solvent

a)

Dissolve

b)

Solubility

c)

Solvent

d)

Solute

7.

In a solution of salt water, _________ is the solvent.

a)

salt

b)

water

8.

In a solution of salt water, the __________ is the solute.

a)

salt

b)

water

9.

It does NOT dissolve in water.

a)

soluble

b)

insoluble

10.

solute + solvent =

a)

solution

b)

equation

11.

Solutes dissolve quicker in _________ water.

a)

cold

b)

warm

12.

Solutes dissolve quicker if you stir them.

a)

true

b)

false

13.

The substance BEING dissolved in a solution.

a)

sands

b)

solute

c)

solvent

d)

alloy

14.
Solubility is defined as
a)
the ability to catch on fire
b)
the ability to be dissolved
c)
the ability to fly.
d)
the ability to get on Mrs. D's nerves.
15.
In this mixture, which of the following will be the solute?
a)
The water in the glass
b)
The glass that holds the final mixture
c)
The solution containing both powder and water
d)
The powder on the spoon
16.

In which beaker does salt dissolves faster?

a)

Hot water

b)

Room temperature

c)

Ice watet

17.
a)

solvent

b)

solute

18.
a)

solvent

b)

solute

19.
Because water has a positive and a negative end, and is attracted to other molecules it is called a ______ molecule.
a)
mickey mouse
b)
polar (tiny magnet)
c)
special
d)
miracle
20.
The property where water can dissolve almost all substances on Earth.
a)
adhesion
b)
capillary action
c)
cohesion
d)
universal solvent
21.
What does "polar" mean?
a)
A molecule is cold
b)
A molecule has ionic bonds
c)
A molecule has covalent bonds
d)
A molecule has areas of positive and negative charge
22.

Hydrogen attractions between water molecules are called

a)

Covalent bonds

b)

Ionic bonds

c)

Polar bonds

d)

Hydrogen bonds

23.

a)

soluble

b)

insoluble

24.

Which of the following would NOT increase the rate at which a sugar cube dissolves?

a)

Reducing the amount of solvent

b)

Crushing the sugar cube

c)

Stirring the solution

d)

Heating the solvent

25.

You can make a solute dissolve more quickly in a solvent by

a)

adding more solute.

b)

adding ice.

c)

heating the solvent.

d)

removing some solvent.

26.
Which of the following would dissolve the slowest?
a)
a sugar cube in hot water
b)
a sugar cube in cool water
c)
powdered sugar in cool water
d)
powdered sugar in hot water
27.

Which of the following would result in being able to dissolve a greater amount of solid in a solution?

a)

Lower the temperature.

b)

Decrease the pressure of the solution.

c)

Increase the pressure of the solution.

d)

Heat the solution.

28.

Stirring the solution...

a)

decrease the rate of solubility

b)

Doesn't change the rate of solubility

c)

increase the rate of solubility

d)

None of the above

29.

When you measure how fast a solute dissolves, you are measuring the

a)

amount of dissolving

b)

rate of particle movement

c)

amount of particle movement

d)

rate of solubility

30.

The smaller the particle size results in a....

a)

increase in solubility

b)

decrease in solubility

c)

decrease in surface area

d)

increase in bond strength

31.
In the above picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)
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
32.

Use the Solubility Rules to determine if the following compound is soluble in water:


MgCl2

a)

Soluble

b)

Insoluble

33.

CaCl2(aq) + 2 AgNO3(aq) → Ca(NO3)2(aq) + 2 AgCl(s)


Which product above is the precipitate?

a)

CaCl2(aq)

b)

AgNO3(aq)

c)

Ca(NO3)2(aq)

d)

AgCl(s)

34.

Which type of solution contains the maximum amount of solute?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

35.

Which type of solution is considered “unstable”?

a)

Supersaturated

b)

Saturated

c)

Unsaturated

36.

Which type of solution has the capability of dissolving more solute without a change in temperature?

a)

Supersaturated

b)

Saturated

c)

Unsaturated

37.

Determine the type of solution present when 60 grams of Ammonia are dissolved at 10°C

a)

Supersaturated

b)

Saturated

c)

Unsaturated

38.

Determine the type of solution present when 70 grams of Ammonium Chloride are dissolved at 90°C

a)

Supersaturated

b)

Saturated

c)

Unsaturated

39.
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
40.

When 40 grams of NaCl is dissolved in 100 grams of water at 90 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

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