AnswersFoothill-B Period-Chemistry-2627BLab: Measuring pH

Equilibria of Acids and Bases Answers

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1
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Which of these refers to the concentration of an acid?

A
a compound that accepts protons
B
an acid that does not dissociate completely when placed in water
C
an intrinsic characteristic of a particular acid related to its dissociation constant
D
a measure of quantity of acid dissolved in water that is designated by molarity
2
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What does it mean for a weak acid to be in equilibrium?

A
The acids only slightly dissociate and readily undergo reverse reaction.
B
The position of equilibrium in weak acids lies more to the right than to the left.
C
At equilibrium there is a small amount of HA and more and .
Option C
D
At equilibrium there is the same amount of HA, and .
Option D
3

Which is true of weak acids and bases?

A
They partially dissociate in water.
B
They dissociate completely in water.
C
They are unable to react with water.
D
They lose all their properties when in water.
4

Which of these accurately describes why an acid is strong?

A
An acid is strong when it undergoes a reverse reaction.
B
An acid becomes strong when it is mixed with a base.
C
An acid’s strength is due to the amount present in a solution.
D
An acid is strong when it dissociates completely in water.
5

Which equations shows the complete dissociation of a strong base?

A
mc012-1.jpg
Option A
B
mc012-2.jpg
Option B
C
mc012-3.jpg
Option C
D
mc012-4.jpg
Option D
6

Which statement best relates the strength and concentration of a base?

A
At high enough concentrations, a weak base becomes strong.
B
Even at low concentrations, a strong base is strong.
C
A weak base always has a low concentration.
D
The stronger the base, the higher its concentration.
7

If hydrofluoric acid is a stronger acid than acetic acid, which statement is most likely true?

A
The conjugate acid of hydrofluoric acid is weaker than that of acetic acid.
B
The conjugate acid of hydrofluoric acid is stronger than that of acetic acid.
C
The conjugate base of hydrofluoric acid is weaker than that of acetic acid.
D
The conjugate base of hydrofluoric acid is stronger than that of acetic acid.
8

What does it mean for a strong acid to be in equilibrium?

A
The equilibrium lies far to the right so that products are very heavily favored.
B
The equilibrium lies far to the left so that reactants are heavily favored.
C
At equilibrium the products and the reactants are in equal balance.
D
At equilibrium there are a lot of strong acids and very few ions.
9

The Ka of an acid is 1.3 10–7. Based on the Ka and its relationship with Kw, what is the value of Kb?Use .

Question illustration
A
1.3 10–21
Option A
B
7.7 10–15
Option B
C
1.3 10–14
Option C
D
7.7 10–8
Option D
10

Look at the table of dissociation constants for some acids.Acid KaAcetic acidChlorous acidNitrous acidPropionic acidWhich of these is the strongest acid?

Question illustration
A
acetic acid
B
chlorous acid
C
nitrous acid
D
propionic acid
11

How does the value of and compare with the concentrations of hydronium ion and hydroxide ion?

Question illustration
A
mc019-3.jpg
Option A
B
mc019-4.jpg
Option B
C
mc019-5.jpg
Option C
D
mc019-6.jpg
Option D
12

A base is added to water. What happens when the position of equilibrium lies to the left?

A
The base is completely dissociating into products.
B
The base is partially dissociating into products.
C
The base is not dissociating into any ions.
D
The base is present in very small amounts.
13

If the base-dissociation constant, Kb, for a substance is 4.3 10–10, what does this tell you about Ka?Use .

Question illustration
A
Ka = 2.3 10–5
Option A
B
Ka = 1.0 10–4
Option B
C
Ka = 2.3 102
Option C
D
Ka = 1.0 103
Option D
14

A solution conducts an electric current more easily when the solution contains more ions. An acidic solution conducts an electric current very easily. What type of acid is in this solution?

A
a weak acid because it dissociates completely
B
a strong acid because it dissociates completely
C
a weak acid because it dissociates partially
D
a strong acid because it dissociates partially
15

An acid has a molarity of 0.01 M. What does the 0.01 M refer to?

A
the strength of the acid
B
the concentration of the acid
C
the amount of base present in the acid
D
the amount of base needed to neutralize the acid

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