Question 1

Marks: 1

Which of the following statements is incorrect about 0.01 mol dm^–3 CH₃COOH?

the pH = 2
[H⁺] << 0.01 mol dm^–3
[CH₃COO^–] is approximately equal to [H⁺]
CH₃COOH is partially ionized

Question 2

Marks: 1

Two flasks contain two different acids labelled as HA and HB. A student measures the pH of each flask, and finds that they are pH 1 and pH 3 respectively. Which of the following statements is true?

HA is a stronger acid than HB
HB is a stronger acid than HA
The [H₃O⁺] in the solution of HB is 3 times greater than the [H₃O⁺] in the solution of HA.
The [H₃O⁺] in the solution of HA is 100 times greater than the [H₃O⁺] in the solution of HB.

Question 3

Marks: 1

Which of the following solutions will have the largest amount of H⁺ ions in moles?

20 cm³ of 2.0 mol dm⁻³ sulfuric acid
10 cm³ of 3.0 mol dm⁻³ nitric acid
80 cm³ of 0.5 mol dm⁻³ hydrochloric acid
40 cm³ of 1.0 mol dm⁻³ ethanoic acid

Question 4

Marks: 1

If the pH of two acids, X and Y, are pH 1 and pH 2 respectively, which of the following is true?

X and Y could be strong or weak acids
The concentration of [H⁺] ions in X is higher than in Y
Acid X is stronger than acid Y

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

Question 5

Marks: 1

A student has two flasks containing 150 cm³ of nitric acid, HNO₃(aq) and ethanoic acid, CH₃COOH(aq). She writes the following three statements in her notebook about the acids. Which of them are correct?

HNO₃ dissociates more than CH₃COOH
HNO₃ conducts electricity better than CH₃COOH
more NaOH can be neutralized with HNO₃ than CH₃COOH

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

Question 6

Marks: 1

Which row shows the correct colours for two common indicators used in acid-alkali titrations?

phenolphthalein

methyl orange

	colour in acid	colour in alkali	colour in acid	colour in acid
A	pink	colourless	yellow	red
B	colourless	pink	yellow	red
C	pink	colourless	red	yellow
D	colourless	pink	red	yellow

Question 7

Marks: 1

In a titration, the equivalence point is reached when 23.70 cm³of 0.02 mol dm^-3 potassium hydroxide reacts with 0.03 mol dm^-3 of sulfuric acid. What volume of acid is needed?

$\frac{2 \times 0.02 \times 23.70}{0.03}$
$\frac{0.03}{2 \times 0.02 \times 23.70}$
$\frac{0.02 \times 23.70}{0.03}$
$\frac{0.03 \times 23.70}{2 \times 0.02}$

Question 8

Marks: 1

What is the number of moles of barium hydroxide in a 100 cm³ solution with a pH of 11 at 25 ℃?

(K_w = 1.00 x 10^-14 mol² dm^-6 at 298 K)

1 $\times$ 10^-11 mol
1 $\times$ 10^-3 mol
0.5 $\times$ 10^-3 mol
0.5 $\times$ 10^-4 mol

Question 9

Marks: 1

What is the pH of a solution made by adding 6.0 g of sodium hydroxide to 1 dm³ of water at 298K? (M_r NaOH = 40.0)

(K_w = 1.00 x 10^-14 mol² dm^-6 at 298 K)

-log $(\frac{{6.0 \times 10}^{- 14}}{40.0})$
-log $(\frac{{40.0 \times 10}^{- 13}}{6.0 \times 1000})$
-log $(\frac{{4.0 \times 10}^{- 15}}{6.0})$
-log $(\frac{{4.0 \times 10}^{- 13}}{6.0})$

Question 10

Marks: 1

Which values are correct for a solution that contains 0.056 g of KOH (M_r= 56) in 100 cm³ of water?

(K_w = 1.00 x 10^-14 mol² dm^-6 at 298 K)

[H⁺] = 1.0 10^-2 mol dm^-3 and pH = 2.00
[OH^-] = 1.0 10^-2 mol dm^-3 and pH = 2.00
[H⁺] = 1.0 10^-12 mol dm^-3and pH = 12.00
[OH^-] = 1.0 10^-12 mol dm^-3and pH = 2.00

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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