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pH review

Total questions: 45

Worksheet time: 1hrs 19mins

Name
Class
Date
1.

How much KNO3 solute is saturated at 40 degrees?

a)

75 grams

b)

55 grams

c)

65 grams

d)

85 grams

2.

How much Ce2(SO4)3 solute is saturated at 80 degrees?

a)

20 grams

b)

15 grams

c)

30 grams

d)

2 grams

3.

What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

4.

What type of a solution is 20g NaCl at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

5.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
6.
Which of these solutes does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
7.

Which of the following affect solubility?

a)

how big the particles are

b)

size of the beaker

c)

temperature of solvent

d)

how much you stir or shake the solution

8.

When making kool aid, the flavor mix is the

a)

solute

b)

solvent

9.

When making kool aid the water is the

a)

solute

b)

solvent

10.

What is the molarity of 3 mole of hydrochloric acid (HCl) in 3 L of water. 

a)
3
b)
1
c)
6
d)
9
11.

What is the molarity of 4 grams of sodium chloride (NaCl) in 3,800 mL of solution?

a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
12.

How many L are required to make 3.5 M hydrochloric acid (HCl) using 1.1 moles? 

a)
3.18 L
b)
0.31 L
c)
3.85 L
d)
4.6 L
13.

How do you convert mL to L

a)

mL x 1000

b)

mL/1000

14.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

15.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

16.

A measure of how much solute is dissolved in solution or "strength" of solution is called......

a)

concentrated

b)

concentration

c)

dilute

d)

dilution

17.

What is the molarity of 0.50 moles of NaCl in 0.25 L of solution

a)

1 M

b)

1/2 M

c)

2 M

d)

1.5 M

18.

The lower the molarity, the ________ the number of particles in the solution

a)

fewer

b)

greater

19.

The higher the molarity, the ________ the solution

a)

more concentrate

b)

less concentrated

20.

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

21.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

22.

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

23.

If you have 34 mL of a 0.5 M NaBr solution, what will the concentration be if 56 mL of water is added to it (add both volumes together for V2)?

a)

.189 M

b)

3.78 M

c)

.389 M

d)

1.76 M

24.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
25.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
26.
Which solution releases H+ in solution?
a)
Base
b)
Acid
c)
Buffer
d)
Water
27.
A solution with a pH of 3.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
28.
This substance releases OH- into solution
a)
Acid
b)
Base
c)
Neutral
29.

If a solution has a pOH of 3.7 the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

30.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

31.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.60

b)

2.5

c)

5.0

d)

7

32.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

33.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

34.
Strong acids and bases...
a)
do not break apart into ions (non-electrolyte)
b)
partially break apart into ions (weak electrolyte)
c)
completely break apart into ions (non-electrolyte)
d)
completely break apart into ions (strong electrolyte)
35.
If an acid is combined with a base of equal strength, the result will most likely be
a)
a neutral solution.
b)
a stronger acid.
c)
impossible to tell without testing the pH.
d)
a stronger base
36.

Identify the following chemical:

HCl

a)

Acid

b)

Arrhenius base

c)

Bronsted-Lowry base

d)

Salt

37.

Identify the following chemical:

HNO3

a)

Acid

b)

Arrhenius base

c)

Bronsted-Lowry base

d)

Salt

38.

Identify the following chemical:

NaOH

a)

Acid

b)

Arrhenius base

c)

Bronsted-Lowry base

d)

Salt

39.

Identify the following chemical:

LiOH

a)

Acid

b)

Arrhenius base

c)

Bronsted-Lowry base

d)

Salt

40.

Identify the following chemical:

Ba(OH)2

a)

Acid

b)

Arrhenius base

c)

Bronsted-Lowry base

d)

Salt

41.

Identify the following chemical:

CaCl2

a)

Acid

b)

Arrhenius base

c)

Bronsted-Lowry base

d)

Salt

42.

What type of compound is NaCl?

a)

Acid

b)

Arrhenius Base

c)

Salt

d)

Bronsted-Lowry Base

43.
Tastes Sour
a)
Acids
b)
Bases
c)
Salts
d)
All
44.

Which properties are acids? (select all that apply)

a)

Taste sour

b)

Feels slippery

c)

Reacts with metals to produce hydrogen (H)

d)

Turns methyl red to yellow

e)

Turns litmus red

45.

Which properties are bases? (select all that apply)

a)

Taste bitter

b)

Feels slippery

c)

Reacts with metals to produce hydrogen (H)

d)

Turns methyl red to yellow

e)

Turns litmus blue

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