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Chemistry Test #7 Review

Total questions: 70

Worksheet time: 6hrs 50mins

Name
Class
Date
1.

Which 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

2.

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.

3.

A solution that contains all of the solute it can hold at a given temperature is

a)

diluted.

b)

saturated.

c)

supersaturated.

d)

unsaturated.

4.

The amount of solute that can be dissolved in a specific amount of solvent at a given temperature is its

a)

concentration.

b)

density.

c)

dilution.

d)

solubility.

5.

Three 10 g samples of sugar are represented below.


Sample A dissolves in water more slowly than sample B.

Sample B dissolves more slowly than sample C.

Which of the following best explains why sample A dissolves more slowly than the other two?

a)

It has the most volume.

b)

It has the smallest surface area.

c)

It has the largest number of sugar molecules.

d)

It has the fewest bonds between sugar modules.

6.

A technican prepared a solution by heating 100 mL of distilled water while adding KCl crystals until no more KCl would dissolve. She then capped the clear solution and set it aside on the lab counter. After several hours she noticed the solution had become cloudly and some solid had settled to the bottom of the flask. Which statement best describes what happened?

a)

As the solution cooled, evaporation of water increased the KCl concentration beyond its solubility.

b)

Water molecules, trapped with the KCl crystals, were released after heating.

c)

At lower temperatures the solubility of KCl decreased and recrystallization occurred.

d)

At increased temperatures the solubility of KCl increased and remained too high after cooling.

7.

A student pours mineral salts into a bottle of cold water. Which of the following best explains why shaking the bottle will affect the dissolving rate of the salt?

a)

Shaking exposes the salts to the solvent more quickly.

b)

Shaking helps more water evaporate.

c)

Shaking equalizes the water temperature.

d)

Shaking causes more ions to precipitate out of solution.

8.

Students in Ms. Alvarez’s science class are investigating how temperature, in degrees Celsius (C), affects the solubility of a compound in 100 milliliters (mL) of water. Ms. Alvarez provides the students with a graph that shows the solubility of a certain compound, as shown below.


She then tell the students that she will demonstrate how many grams (g) of the compound will dissolve in 100 mL of water at 40 C. Based on the information in the graph, which of the following is the best prediction of how many grams of the compound will dissolve at 40 C?

a)

40 g

b)

65 g

c)

85 g

d)

100 g

9.

The solubility graph below shows the amounts of four substances that will dissolve in 100 grams of water at various water temperatures.


Which substance has 80 grams of solute dissolved in 100 grams of water at 50 C?

a)

Potassium Bromide

b)

Ammonium Chloride

c)

Potassium Chloride

d)

Lithium Hydroxide

10.

A solution that is able to dissolve additional solute is best described as

a)

supersaturated.

b)

concentrated.

c)

saturated

d)

unsaturated.

11.

The substance being dissolved is called the ________

a)

solvent

b)

solid

c)

solute

d)

solvate

12.

Gases are more soluble at ______temps and _____pressures

a)

high, low

b)

low , high

c)

high, high

d)

low, low

13.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

14.

Molarity is defined as _________ divided by ___________

a)

mol, liters

b)

mol, kg

c)

kg, liters

d)

liters, kg

15.

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

16.
What is the unit for molarity?
a)
mass/liters
b)
moles
c)
liters
d)
moles/liter
17.
A measure of the amount of solute in a given amount of solvent or solution is...
a)
saturated
b)
solubility
c)
concentration
d)
miscible
18.
A saturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
19.
A supersaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
20.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
21.
The dissolving medium in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
22.
What is the molarity of a 2 liter solution containing 5 moles of NaCl?
a)
2.5
b)
0.4
c)
2.5 moles/liter
d)
10 moles/liter
23.
How many moles of NaCl are present in 6000. ml a 1.5 M NaCl solution?
a)
9 moles NaCl
b)
9000
c)
9
d)
4000  moles NaCl
24.
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
25.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
26.
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
27.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
28.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
29.
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
30.
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
31.

How do you know when you have a saturated solution?

a)

You don't see anymore material in the solution. It has dissolved.

b)

The material dissolves and no more will dissolve because you see it collect at the bottom.

c)

The solution is bubbling and cloudy.

d)

The solution is clear and there is nothing at the bottom.

32.
A questions asks, "what volume of 0.125 M KMnO4 is required to yield 0.180 mol of potassium permanganate,
KMnO4?"  What is the correct formula set up to solve for this problem?
a)
.125 M = .180 mol / L
b)
M1 V1 = M2 V2
c)
.125 M = L / .180 mol
d)
none of the choices listed
33.
A sample of 0.0255 mol potassium hydroxide, KOH, was dissolved in water to yield 10.0 mL of
solution.  Which amount would you need to change to solve for molarity?
a)
change .0255 moles to grams
b)
change 10 mL to L
c)
change both values to grams and L
d)
leave it as it is
34.
Which formula should you use to convert 2.00 L of 0.300 M sulfuric acid, how many mL of a 1.00 M stock solution should be
used?
a)
molarity formula
b)
dilution formula
c)
both will work
d)
neither will work
35.
Which of the following would result in being able to dissolve a greater amount of gas in a
solution?
a)
Heat the gas and solution
b)
Decrease the pressure of the solution
c)
Make the gas an electrolyte
d)
Cool the gas and solution
36.
90 grams of sodium nitrate (NaNO3) are put into 100 grams of water and stirred. The final
mixture has a temperature of 20°C. About how many grams of the sodium nitrate dissolved?
a)
23
b)
73
c)
80
d)
88
37.
Which of the following would decrease the rate of solution when dissolving a solid in water?
a)
Raise the temperature of the solution
b)
Crush the solid before mixing
c)
Stir the solution after mixing
d)
Use a single cube of solid
38.
Which of the following is the best way to determine if an aqueous solution  is supersaturated?
a)
add more solvent
b)
measure the temperature
c)
filter out excess solute
d)
add a seed crystal
39.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
40.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
41.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
42.
Molarity is measured in
a)
moles per kg
b)
mols per L
c)
moles per kJ
d)
moles per mL
43.
How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 
a)
3.18 L
b)
0.31 L
c)
3.85 L
d)
4.6 L
44.

If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?

a)

20.9 mol

b)

21 mol

c)

0.07 mol

d)

0.0209 mol

45.
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
46.
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
47.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
48.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
49.
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
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.

How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?

a)

27.8 mL

b)

0.0278 mL

c)

360 mL

d)

278 mL

52.
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
53.

A dilution is when

a)

solute is added to the volume of solution

b)

water is added to the volume of solution

c)

solute is removed from the volume of solution

d)

water is removed from the volume of solution

54.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250.0 mL?

a)

15.9 M

b)

0.636 M

c)

0.642 M

d)

1.59 M

55.

If I dilute 250 mL of 0.10 M lithium acetate solution to a volume of 750 mL, what will the concentration of this solution be?

a)

2 M

b)

0.02 M

c)

0.033 M

d)

0.08 M

56.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

57.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

58.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
59.
If the [OH-] of a solution is 2.7 x 10-4 mol/L the pOH of the solution is
a)
10.44
b)
3.56
c)
1.00
d)
-4.43
60.
If the [H+] of a solution is 6.8 x 10-9 mol/L the pH is
a)
8.17
b)
8.2
c)
9.99
d)
8.62
61.

What pH range would you get for an acid?

a)

0-6

b)

7

c)

7-14

d)

2-10

62.
How do acidic solutions taste?
a)
Delicious
b)
Sweet
c)
Bitter
d)
Sour
63.

​ (a)   conduct electricity and turn litmus paper red.

Choose from the below words
Acids
Bases
Neutral solutions
Salts
64.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
65.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

66.

What is the concentration of a HCl solution if 24.7 cm3 of HCl are completely neutrilized by 35.8 cm3 of a 0.25 M NaOH solution?

a)

0.362 M

b)

3.62 M

c)

0.172 M

d)

35.4 M

67.

What mass of KHP will be completely neutrilized by 32.57 cm3 0.175 M standard NaOH solution? The Molar Mass of KPH is 204.22 g/mol.

a)

23.28 g KHP

b)

1.164 g KHP

c)

11.64 g KHP

d)

2.328 g KHP

68.

If it takes 54 cm3 of 0.1 M NaOH to neutralize 125 cm3 of an HCl solution, what is the concentration of HCl?

a)

0.043 M

b)

23.148 M

c)

0.231 M

69.

If it takes 25 cm3 of 0.05 M HCl to neutralize 345 cm3 of NaOH solutions, what is the concentration of the NaOH solution?

a)

0.004 M

b)

276 M

c)

0.036 M

70.

What is the equivalence point of a titration?

a)

Where the amount of acid and base are balanced according to the equation

b)

Where there is no base

c)

At the end

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