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Acid/Base Honors Review

Total questions: 60

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

2.

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

3.

The pH of a solution is 8.43. What is the [H3O+]concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

4.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

5.

If the pH of a solution is 8 the [H3O+] is

a)

1.0 x 106 M

b)

8.0 x 101 M

c)

1.0 x 108 M

d)

1.0 x 10-8 M

6.

If the [OH-] of a solution is 2.7 x 10-4 M, the pOH of the solution is

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

7.

If the [H3O+] of a solution is 6.8 x 10-8 M, the pH is

a)

7.17

b)

3.2 x 10-5

c)

7.2

d)

7.62

8.

If the [H3O+] of a solution is 9.3 x 10-3 M, the pOH of the solution will be

a)

2.03

b)

1.02

c)

11.97

d)

12.98

9.

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

10.

Oranges have a [H3O+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

11.

Ammonia has a pOH of 2. Ammonia is a(n) __________.

a)

acid

b)

base

c)

neutral

d)

metal

12.

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

13.

What is the pOH of a solution with [H+] = 1.24 x 10 -2?

a)

1.91

b)

1.61

c)

12.09

d)

12.39

14.

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

15.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-14 M

c)

1.0 x 10-4 M

d)

1.0 x 10-7 M

16.

What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?

a)

-1.14

b)

1.14

c)

2.01

d)

11.99

17.

What is the [OH-] if the [H+] is 1.0 x 10-3M?

a)

1.0 x 10-3 M

b)

1.0 x 10-14 M

c)

6.02 x 10-23 M

d)

1.0 x 10-11 M

18.

What is the [OH-] if the pH is 4.9?

a)

4.9 x 10-10 M

b)

1.0 x 10-4 M

c)

1.25 x 10-5 M

d)

7.94 x 10-10 M

19.

A 1.0 x 10-4 M solution of HNO3 has a [H+] concentration of: (Notice HNO3 has one H+.)

a)

1.0 x 10-14

b)

log 1.0 x 10-4

c)

1.0 x 10-10

d)

1.0 x 10-4

20.

A solution of KOH is 2.5 x 10-5 M. What is the [H+] concentration? (Hint: Find pOH, then pH, then [H+].)

a)

4.60

b)

9.40

c)

3.98 x 10-10

d)

1.0 x 10-4.60

21.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

22.

An Arrhenius base:

a)

donates H+

b)

accepts H+

c)

produces H+

d)

produces OH-

23.

An Arrhenius acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

24.
A hydrogen ion, H+, is the same as a(n):
a)
neutron
b)
electron
c)
proton
d)
hydroxide ion
25.
Forms a OH- hydroxide ion
a)
Lewis Base
b)
Arrhenius Base
c)
Bronsted Lowry Base
d)
Bronsted Lowry Acid
26.
The following statement is true for arrhenius acid and base EXCEPT
a)
Arrhenius acid produces H+ ions
b)
Arrhenius base produces OH- ions
c)
H2O need to be present for arrhenius acid base to dissociate
d)
Hydrogen atoms that make the solution acidic
27.

A Bronsted Lowry base:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

28.

Which of the following does not describe an Arrhenius or Bronsted Lowry acid or base?

a)

Produces H+

b)

Produces OH-

c)

Donates H+ to another substance

d)

Donates OH- to another substance

29.

In which of the following aqueous solutions does the weak acid exhibit the highest percentge of ionization?

a)

.01 M HC2H3O2 . (Ka 1.8 x 10 -5)

b)

.01 M HNO2 . ( Ka =4.5 x 10 -4)

c)

.01 M HClO . (Ka= 3.0 x 10 -8)

d)

.01 M HF (Ka= 6.8 x 10 -4)

30.

Z- is a weak base. An aqueous solution of NaZ is prepared by dissolving 0.350 mol of NaZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 8.93 at 25.0 0C. What is the Kb of the solution?

a)

1.2 x 10-5

b)

6.9 x 10 -9

c)

2.1 x 10 -10

d)

2.8 x 10 -12

31.
According to Bronsted-Lowry acid base theory, an acid is a.....
a)
Proton donor
b)
Proton acceptor
c)
Produces H+ when added to water
d)
Made of H+
32.
Which reactant in the following equation is a Bronsted acid?
a)
ammonium
b)
ammonia
c)
hydroxide
d)
water
33.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
34.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)

Cl-

35.

Acetic Acid is a weak monoprotic acid. It's concentration is 0.20M and it's equilibrium concentration of H+ ions is 0.0019M. Calculate it's Ka value.

a)

1.8x10 -5

b)

1.8x10 -15

c)

.0019

d)

5.56x10 -10

36.

Formic Acid is a weak monoprotic acid. It's initial concentration is 0.10M and it's equilibrium concentration of H+ ions is 0.0042M. Calculate it's Ka value.

a)

.150

b)

12.56x10 -6

c)

1.8x10 -4

d)

None of these are correct

37.

Isobutlyamine is a weak base. It's initial concentration is 0.55M and it's equilibrium concentration of OH- ions is 0.0040M. Calculate it's Kb value.

a)

.055

b)

4.0x10 -3

c)

1.6x10 -5

d)

3.1x10 -4

38.

Gallic Acid is a weak monoprotic acid. It's concentration is 0.280M and it's equilibrium concentration of H+ ions is 0.0033M. Calculate it's pH value.

a)

3.9x10 -5

b)

4.96

c)

2.48

d)

.280

39.

Uric Acid is a weak monoprotic acid. It's initial concentration is 0.110M and it's equilibrium concentration of H+ ions is 0.034M. Calculate the final concentration of Uric acid.

a)

.011

b)

.034

c)

.076

d)

1.47

40.

Acetic Acid is a weak monoprotic acid. It's concentration is 0.20M and it's Ka value is 1.8x10 -5. Calculate it's pH value.

a)

.698

b)

2.72

c)

11.28

d)

None of the answers are correct

41.

Trimethyamine is a weak base. It's concentration is 0.390M and it's equilibrium concentration of OH- ions is 0.0044M. Calculate it's pH value.

a)

2.36

b)

11.6

c)

.410

d)

None of the above are correct

42.

Ammonia is a weak base. It's concentration is 0.150M and it's Kb value is 1.7x10 -5. Calculate it's pH value.

a)

2.80

b)

11.2

c)

Both answers are correct

d)

None of the above are correct

43.

Butylamine is a wack base. It's concentration is 0.230M and it's equilibrium concentration of OH- ions is 8.6x10 -6M. Calculate it's Kb value and pOH.

a)

3.2x10 -10 and 9.49

b)

8.6x10 -10 and 9.07

c)

3.2x10 -10 and 4.93

d)

None of the above

44.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
45.

A type of chemical that forms solutions that taste sour, due to high concentrations of positive hydrogen ions

a)

acid

b)

base

c)

salt

d)

pH

46.

What is considered to be in the middle of the pH scale

a)

acidic

b)

neutral

c)

basic

d)

indicator

47.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
48.
In a ____ reaction, an acid and a base produce a salt and a water. 
a)
concentrated
b)
decomposition
c)
dilute
d)
neutralization
49.
Forms hydroxide ions (OH-) in water
a)
Acids
b)
Bases
c)
All
50.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
51.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
52.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
53.
I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
54.
Identify the products of the chemical equation
3 LiOH + H3PO4 →
a)
Li3PO4 + 3 H2O
b)
LiPO4 + 3 H2O
c)
Li(PO4)3 + 3 H2O
d)
BOY + La + N2
55.
What acid and what base would you choose to prepare the salt potassium chlorate?
a)
KOH and HClO3
b)
KOH and HClO2
c)
HK and OHClO3
d)
HK and OHClO2
56.
If phenolphthalein turns bright pink, it indicates
a)
an acid 
b)
a base
c)
a neutral
57.
What does pH measure?
a)
Amount of Oxygen Ions
b)
Amount of Hydrogen Ions
c)
The amount of salt in a solution
d)
The density
58.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
59.

What allows us to know when the end point has been reached?

a)

Bubbles

b)

Feels warm

c)

indicator changing color

d)

Turns to a solid

60.

If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? (record you answer with the correct unit)

a)

0.043 M

b)

0.034 M

c)

0.065 M

d)

0.77 M

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