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Quiz 4/8-4/9

Total questions: 35

Worksheet time: 45mins

Name
Class
Date
1.
Which of the following shows the correct dissolution reaction for BaCl2?
a)
Ba 2+(aq) + Cl2-(aq) -> BaCl2(s)
b)
BaCl2(aq) -> Ba 2+(aq) + 2Cl-(aq)
c)
 BaCl2(s) -> Ba 2+(aq) + 2Cl-(aq)
d)
Ba 2+(aq) + 2Cl-(aq) -> BaCl2(s)
2.
If K < Q, which part of the reaction will speed up?
a)
forward
b)
reverse
c)
none
3.
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
a)
2.9 x 10-5 M
b)
5.7 x 10-5 M
c)
9.4 x 10-5 M
d)
3.7 x 10-5 M
4.
The molar solubility of PbI2 is 1.52 x 10-3 M. Calculate the value of Ksp for PbI2.
a)
3.51 x 10-9
b)
1.40 x 10-8
c)
4.62 x 10-6
d)
1.52 x 10-3
5.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
6.
The pH at the equivalence point of the titration of a strong acid with a strong base is:
a)
3.9
b)
4.5
c)
7.0
d)
8.2
7.
Silver chromate, Ag2CrO4, has a Ksp of 8.96 x 10-12. Calculate the solubility in mol/L of silver chromate.
a)
1.31 x 10-4M
b)
1.65 x 10-4M
c)
2.25 x 10-12M
d)
2.08 x 10-4M
8.
The pH of a solution at 25ₒC in which [OH-] = 3.9 x 10-5M is:
a)
4.41
b)
3.90
c)
9.59
d)
4.80
9.
Calculate the pH of a 0.47M NH3 (Kb = 1.8 x 10-5) solution.
a)
2.54
b)
8.93
c)
5.07
d)
11.46
10.
The solubility of CaSO4 in pure water at 0ₒC is 1.14 g/L. The value of the solubility product is
a)
8.37 x 10-3
b)
1.14 x 10-3
c)
9.15 x 10-2
d)
7.01 x 10-5
11.
A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCl is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing?
a)
OH-
b)
Na+
c)
F-
d)
Na-
12.
The correct mathematical expression for finding the molar solubility (s) of Sn(OH)2 is:
a)
2s2 = Ksp
b)
2s3 = Ksp
c)
4s3 = Ksp
d)
8s3 = Ksp
13.
When the chemical reaction A + B ↔ C+ D is at equilibrium,
a)
both the forward and reverse reactions have stopped.
b)
the sum of the concentrations of A and B equals the sum of the concentrations of C and D.
c)
all four concentrations are equal.
d)
neither the forward nor the reverse reactions have stopped.
14.
A substance that ionizes completely in solution is
a)
an insulator.
b)
a strong electrolyte. 
c)
a weak acid.
d)
a non-electrolyte.
15.
When citric acid is produced by the cells of an orange and dissolves in water, it produces a relatively small number of hydronium ions. Citric acid is best described as a
a)
concentrated acid. 
b)
weak acid. 
c)
dilute acid.
d)
strong acid.
16.
Which is the weakest acid?
a)
HF
b)
HNO2
c)
CH3COOH
d)
HClO
17.
Which of the following correctly describes the strengths of the acids in solution?
a)
HA and HB are both examples of strong acids.
b)
HA and HB are both examples of weak acids.
c)
HA is an example of a strong acid, HB is an example of a weak acid.
d)
HA is an example of a weak acid, HB is an example of a strong acid. 
18.

Which one of the following is the solubility product constant for Mn(OH)2?

a)

Ksp = [Mn2+][OH-]2

b)

Ksp = [Mn2+][2 OH-]2

c)

Ksp = [Mn2+]2[OH-]2

d)

Ksp = [Mn2+]2[OH-]

19.

The solubility of HgS is 5.5 x 10-27 mol/L. What is Ksp for HgS?

a)

4.0 x 10-3

b)

8.2 x 10-4

c)

1.3 x 10-13

d)

3.0 x 10-53

20.

Calculate the molar solubility of Fe2S3.

Ksp = 1.4 x 10-88

a)

1.2 x 10-44 M

b)

1.1 x 10-18 M

c)

4.8 x 10-24 M

d)

5.5 x 10-62 M

21.

Calculate the equilibrium constant for the reaction:
CuCl (s) + I- (aq)  ↔\leftrightarrow   CuI (s) + Cl- (aq)
CuCl;  Ksp = 1.9 x 10-7
CuI;  Ksp = 5.1 x 10-12

a)

8.4 x 10-2

b)

2.3 x 10-6

c)

3.7 x 104

d)

4.4 x 1017

22.

For BaSO4, Ksp = 1.1 x 10-10. If you mix 200. mL of 1.0 x 10-4 M Ba(NO3)2 and 500. mL of 8.0 x 10-2 M H2SO4, what will be observed?

a)

A precipitate forms because Qsp > Ksp

b)

A precipitate forms because Qsp < Ksp

c)

No precipitate forms because Qsp < Ksp

d)

No precipitate forms because Qsp > Ksp

23.

A saturated solution of Ca(OH)2, has a pH of 12.40. What is the Ksp for Ca(OH)2?

a)

2.5 x 10-2

b)

1.3 x 10-2

c)

8.0 x 10-6

d)

2.0 x 10-6

24.

The Ksp expression for a saturated solution of Ca3(PO4)2 is

a)

Ksp = [Ca2+][PO43-]

b)

Ksp = [3Ca2+][2PO43-]

c)

Ksp = [Ca2+]3[PO43-]2

d)

Ksp = [3Ca2+]3[2PO43-]2

25.

What will happen if some solid AgNO3 is added to a saturated solution of AgCl ?

a)

The AgNO3 will not dissolve

b)

More solid AgCl will dissolve

c)

More solid AgCl will produced

d)

There will be no effect on AgCl equilibrium

26.

The Ksp value for PbF2 is 4 x 10-8. Calculate the molar solubility of solid PbF2 in a 0.5M NaF solution.

a)

8 x 108

b)

1.6 x 107

c)

8 x 10-8

d)

1.6 x 10-7

27.

A person mixes 100.0 mL of 0.0015M CaCl2 and 50.0 mL of 0.0081M K2SO4. If the Ksp for CaSO4 is 2.4 x 10-5 , will a CaSO4 precipitate be observed?

a)

No precipitate occur

b)

Precipitate occur

28.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
29.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
30.
An element with five valence electrons is
a)
phosphorus
b)
oxygen
c)
beryllium
d)
rubidium
31.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
32.
How many electrons are in the outer (valence) shell of Chlorine (Cl)?
a)
1
b)
3
c)
6
d)
7
33.
What is the name of the group that has the MOST reactive METALS in it?
a)
Alkaline earth
b)
Alkali
c)
transition
d)
actinides
34.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
35.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17

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