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Magnet - Solutions, Acids and Bases Practice Multiple Choice

Total questions: 61

Worksheet time: 7hrs 2mins

Name
Class
Date
1.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
2.
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.
3.
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
4.
The _____is the part that gets dissolved. 
a)
solute 
b)
solvent 
c)
solution 
d)
Sacajawea 
5.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
6.
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
7.
What is the molarity of a solution made from 325.4g of AlCl3 with enough water to make 500.0 mL?
a)
4.88 g
b)
4.88 M
c)
2.440 M
d)
2.44 M
8.
At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?
a)
60 ºC
b)
30 ºC
c)
50 ºC
d)
83 ºC
9.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
10.
When a solution is very concentrated, it has a high amount of _________ to _________.
a)
solute to solvent
b)
solvent to solute
c)
solvent to solution
d)
solution to solute
11.
We can increase the rate a solute will dissolve by 
a)
Heating it, Crushing it Stirring it
b)
Heating it, cooling it crushing it
c)
Stirring it, Crushing it cooling it
d)
Smelling it, crushing it, stirring it
12.

What is the molarity of a solution containing 4.26 g of KCl in 1.25 L of solution? *Change g to mol first, molar mass of KCl = 74.55 g/mol*

a)

3.41 M

b)

0.0457 M

c)

0.0571 M

d)

0.0714 M

13.

Sodium chloride (NaCl) and sucrose (C12H22O11) both dissolve in water. Which solution is able to conduct electricity?

a)

sucrose because it is a covalent molecule and nonelectrolyte

b)

sucrose because it is an ionic compound and electrolyte

c)

sodium chloride because it is an ionic compound and electrolyte

d)

sodium chloride because it is a covalent molecule and nonelectrolyte

14.
How many grams of calcium hydroxide are needed to produce 500. ml of 1.66 M calcium hydroxide solution?
a)
38.7 g
b)
61.5 g
c)
94 g
d)
19.7 g
15.
How much of the 12.0 M stock solution do you need to prepare 250 mls of .20M HCl?
a)
15,000 mls
b)
4.17 mls
c)
9.6 mls
d)
0.0096 mls
16.

Which of the following solutions would contain the highest concentration of hydronium ions, H3O+?

a)

0.10 M HCl

b)

0.10 M HF

c)

0.10 M CH3COOH

d)

0.10 M NaCl

17.
Which of the following word pairs correctly completes the sentence below?
_______ are corrosive substances characterized as having a strong smell, a sour taste, and a _______.
a)
Acids; pH less than 7
b)
Acids; pH greater than 7
c)
Bases; pH greater than 7
d)
Bases; pH less than 7
18.
What would be considered the weakest base? 
a)
8
b)
14
c)
7.8
d)
11.6
19.

What is the pH of a soultion of 0.035 M NaOH

a)

1.46

b)

12.54

c)

2.86 x 10-13

20.

where [H+] and [OH-] are equal

a)

pH=0

b)

pH=14

c)

pH=7

21.
If the pH of a solution is 5 the [H+] is
a)
1.0 x 105  M
b)
1.0 x 109  M
c)
5.0 x 101  M
d)
1.0 x 10-5  M
22.
If the [H3O+] of a solution is 1 x 10-8 mol/L the [OH-] is
a)
1.0 x 10-6
b)
1.0 x 106
c)
1.0 x 10-8
d)
1.0 x 108
23.

Given the equation:

H2SO4 + H2O ↔ H3O+ + HSO4- 1

What is the acid?

a)

H2SO4

b)

H2O

c)

H3O+

d)

HSO4- 1

24.

Given the equation HF + H2O ↔ H3O+ + F-1

Which is the conjugate acid?

a)

HF

b)

H2O

c)

H3O+

d)

F-1

25.

By definition, a Bronsted-Lowry base is a:

a)

proton donor

b)

proton acceptor

c)

Increases the concentration of H3O+

d)

Increases the concentration of OH-

26.

Given the equation:

PO43‑ + H2O ↔ HPO42‑ + OH-

Which species is the conjugate acid?

a)

PO43‑

b)

H2O

c)

HPO42‑

d)

OH-

27.

The term "amphoteric" mean

a)

like an aligator

b)

goes from land to water

c)

behaves like an acid or base

d)

is afraid of reptiles

28.

Given the equation:

NH3 + H2O ↔ OH‑1 + NH4+1

Which species is the conjugate base?

a)

NH3

b)

H2O

c)

OH‑1

d)

NH4+1

29.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
30.
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
31.
The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H2O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if 15.0mL of acid neutralized?
a)
0.8M
b)
1.2M
c)
12.5M
32.
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
33.
A 50.0 mL sample of Ca(OH)2 is neutralized by 300.0 mL of HCl solution with a pH of 1.3. Calculate the molarity of the Ca(OH)2 solution.
a)
1.0 M
b)
0.50 M
c)
0.15 M 
d)
0.30 M
34.

What is this piece of apparatus called

a)

Pipette

b)

Burette

c)

Janette

d)

Cuvette

35.

Which of the following would be a weak base?

a)
b)
c)
d)
36.

How many moles of BaCl2 are formed in the neutralization of 393 mL of 0.171 M Ba(OH)2 with aqueous HCl?

a)

1.15 mol

b)

0.0672 mol

c)

0.0336 mol

d)

2.30 mol

37.

How many moles of HNO3 would be needed to react with 85 mL of 0.75 M KOH?

a)

110 mol

b)

1.1 mol

c)

.11mol

d)

0.064 mol

e)

64 mol

38.

How many mL of 0.50 M HNO3 would be needed to react with 85 mL of 0.75M KOH?

a)

130 mL

b)

0.13 mL

c)

32 mL

d)

0.032 mL

39.

How many grams of water could form in this reaction if 85.0mL of 0.750M KOH are completely neutralized?

a)

1.15g

b)

282g

c)

31.9g

d)

113.g

40.

Solid iron (II) sulfide reacts with hydrochloric acid to form hydrogen sulfide gas and aqueous iron (II) chloride:

FeS (s) + 2 HCl (aq) --> H2S (g) + FeCl2 (aq) If 145 mL of HCl is needed to completely react with 25 g of iron (II) sulfide, what is the concentration of the HCl solution?

a)

3.1 M

b)

0.68 M

c)

2.7 M

d)

9.0M

e)

3.9 M

41.

How many mL of 0.5M HNO3 would be needed to react with 85mL of 0.75M KOH?

a)

127.5mL

b)

0.1275mL

c)

31.9mL

d)

0.031875mL

42.

What is [HCl] if 25.00 mL of HCl neutralizes 20.00 mL of 0.100 M KOH?

a)

0.160 M

b)

0.0800 M

c)

0.0400 M

d)

0.500 M

43.

If 25.0 mL of H3PO4 are neutralized by 42.6 mL of 0.103 M Ca(OH)2, what is [H3PO4]?

a)

0.176 M

b)

0.263 M

c)

0.117 M

d)

0.0585 M

44.

Identify the true statement about the following reaction:

F- + H2O --> HF +OH-

a)

H2O is a bronsted lowry base

b)

H2O is not an acid or base according to either model

c)

H2O is a bronsted lowry acid

d)

H2O is an arrhenius acid

45.

HNO3 + H2O → H3O+ + NO31-

NO31- is the conjugate base of

a)

H2O

b)

HNO3

c)

H3O+

d)

none of the above

46.

Label the acid, base, conjugate acid and conjugate base.

a)acid
b)base
c)conjugate acid
d)conjugate base
1
2
3
4
1)
2)
3)
4)
47.

Click on the conjugate base.

A
B
C
D
48.

Click on the conjugate acid.

A
B
C
D
49.

After a base has accepted an H+ ion, it becomes a(n)

a)

An acid

b)

A Base

c)

A Conjugate Acid

d)

A Conjugate Base

50.

Label the acid, base, conjugate acid and conjugate base.

a)acid
b)base
c)conjugate acid
d)conjugate base
1
2
3
4
1)
2)
3)
4)
51.

What is the conjugate acid of CO3-2?

a)

HCO3

b)

HCO3-

c)

CO2

d)

CO2-

52.

What is NH4+ classified as?

a)

Acid

b)

Base

c)

Conjugate Acid

d)

Conjugate Base

53.

The conjugate acid of HCO3- is ___ and the conjugate base of HCO3- is ___.

a)
H2CO3; CO3-2
b)
CO3-2; CO3-2
c)
H2CO3; H2O
d)
H2O; H2CO3
54.

A Bronsted Lowry base:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

55.

In which of the reactions does HCl donate a proton and thus act as an acid?

a)

A, only

b)

B, only

c)

both A and B

d)

neither A nor B

56.

Which beaker shows a weaker acid?

a)

Beaker B because the substance dissociates less

b)

Beaker A because the substance dissociates less

c)

Beaker B because the substance dissociates more

d)

Both beakers show acids of the same strength

e)

Beaker A because the substance dissociates more

57.

Which beaker shows a stronger acid?

a)

Beaker B because the substance dissociates less

b)

Both beakers show acids of the same strength

c)

Beaker A because the substance dissociates more

d)

Beaker A because the substance dissociates less

e)

Beaker B because the substance dissociates more

58.

Which beaker shows a weaker acid?

a)

Both beakers show acids of the same strength

b)

Beaker B because the substance dissociates more

c)

Beaker A because the substance dissociates more

d)

Beaker B because the substance dissociates less

e)

Beaker A because the substance dissociates less

59.

List the following acids on order of increasing strength:

a)

hydrocyanic, hypochlorous, citric, acetic

b)

acetic, citric, hydrocyanic, hypochlorous

c)

acetic, citric, hypochlorous, hydrocyanic

d)

acetic, hydrocyanic, citric, hypochlorous

60.

List the following acids from strongest to weakest:

a)

hydrocyanic, hypochlorous, citric, acetic

b)

acetic, citric, hydrocyanic, hypochlorous

c)

acetic, citric, hypochlorous, hydrocyanic

d)

acetic, hydrocyanic, citric, hypochlorous

61.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-

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