Question 1

Marks: 1

Four 1.0 M solutions of HCl, NH₃, NaOH and CH₃COOH have been mislabelled, but a student has a pH meter to test the pH of the solutions. Arrange the solutions in order of increasing pH:

HCl (aq) < NH₃ (aq) < NaOH (aq) < CH₃COOH (aq)
CH₃COOH (aq) < HCl (aq) < NH₃ (aq) < NaOH (aq)
HCl (aq) < CH₃COOH (aq) < NH₃ (aq) < NaOH (aq)
NaOH (aq) < NH₃ (aq) < CH₃COOH (aq) < HCl (aq)

Question 2

Marks: 1

Below are four statements about acid and bases. Which is the correct one?

Strong acids are good proton donors and have weak conjugate bases.
Strong bases are good proton donors and have weak conjugate acids.
Weak acids are poor proton acceptors and have strong conjugate bases.
Strong acids are good proton donors and have strong conjugate bases.

Question 3

Marks: 1

Which statement is correct about the action of weak acids and their conductivity?

Weak acids are proton donors and their solutions are good conductors.
Weak acids are proton donors and their solutions are poor conductors.
Weak acids are proton acceptors and their solutions are good conductors.
Weak acids are proton acceptors and their solutions are good conductors.

Question 4

Marks: 1

Which is the correct expression for the ionic product of water at 25 ℃ is

$K_{w} = \frac{[H^{+}] [O H^{-}]}{[H_{2} O]}$
H₂O (l) ⇌ H⁺ (aq) + OH^- (aq)
K_w = [H⁺][OH^-]
1 x 10^-14 mol² dm^-6

Question 5

Marks: 1

34.3 cm³ of 0.125 mol dm^-3 sodium hydroxide solution reacts with 26.0 cm³ of sulfuric acid. What is the concentration of the acid?

$\frac{34.3 \times 0.125}{26.0}$
$\frac{2 \times 34.3 \times 0.125}{26.0}$
$\frac{34.3 \times 0.125}{2 \times 26.0}$
$\frac{26.0}{2 \times 34.3 \times 0.125}$

Question 6

Marks: 1

90 cm³ of water is added to 10 cm³ of sulfuric acid with a pH of 2. What is the new pH of the acid?

1
3
5
7

Question 7

Marks: 1

Which of the following is true about weak acids?

They are poor conductors of electricity
They have a high pH
They react with carbonates to produce carbon dioxide

I and II only
I and III only
II and III only
I, II and III

Question 8

Marks: 1

Which is true about 1.0 mol dm^-3solutions of weak and strong acids?

Magnesium will react with strong acids but not weak acids
Fewer moles of base are needed to neutralise weak acids
Sodium carbonate reacts more slowly with weak acids
Weak acids have a lower pH than strong acids

Question 9

Marks: 1

Four solutions, K, L, M and N have the following properties

K: pH= 8 L: [H⁺] = 1 x 10^-3mol dm^-3 M: pH= 5 N: [H⁺] = 1 x 10^-7mol dm^-3

What is their correct order of increasing acidity?

K < L < M < N
N < L < M < K
K < N < M < L
N < M < L < K

Question 10

Marks: 1

Two beakers contain solutions of hydrochloric acid at pH = 2 and pH = 4. How does the concentration of hydrogen ions compare in the two beakers?

Twice as large
Half as much
$\frac{1}{10}$ of the value
$\frac{1}{100}$ of the value

DP IB Chemistry: SL

Topic Questions

8.2 More About Acids

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

Question 9

Question 10

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