Question 1a

Marks: 1

a)

Using section 22 of the data booklet, identify an indicator that would show a yellow colour in ammonia solution?

[1]

Key Concepts

Acid-Base Titrations

Question 1b

Marks: 2

b)

Suggest two characteristics that make a good indicator for a titration?

[2]

Key Concepts

Acid-Base Titrations

Question 1c

Marks: 1

c)

A typical set of acid-base titration results in shown in the table.

	Rough	Run 1	Run 2
Initial burette reading /+0.05 mL	0.00	0.30	0.60
Final burette reading/ +0.05 mL	24.15	22.55	22.95

Determine the mean volume from these results.

[1]

Key Concepts

Acid-Base Titrations

Question 1d

Marks: 1

d)

What is the recorded uncertainty on the mean volume calculated in part c)?

[1]

Key Concepts

Acid-Base Titrations

Question 2a

Marks: 1

a)

State the relationship between pH and hydrogen ion concentration.

[1]

Key Concepts

pH & [H⁺]

Question 2b

Marks: 1

b)

Determine the pH of 0.200 mol dm^-3 hydrochloric acid.

[1]

Key Concepts

pH & [H⁺]

Question 2c

Marks: 1

c)

Determine the hydrogen ion concentration in a sample of lake water of pH 5.60.

[1]

Key Concepts

pH & [H⁺]

Question 2d

Marks: 1

d)

The table below shows the hydrogen ion concentration in three solutions:

	P	Q	R
[H⁺]	0.001	1 x 10^-5	1.00

List the three solutions in order from low pH to high pH

[1]

Key Concepts

Interpreting pH

Question 3a

Marks: 1

a)

State what is meant by the ionic product of water.

[1]

Key Concepts

The Ionic Product of Water

Question 3b

Marks: 1

b)

Calculate the concentration of [H⁺] in a solution of sodium hydroxide, NaOH, whose concentration is 0.001 mol dm^-3.

[1]

Key Concepts

The Ionic Product of Water
Acid-Base Calculations

Question 3c

Marks: 1

c)

Calculate the pH of 0.001 mol dm^-3 NaOH solution.

[1]

Key Concepts

Acid-Base Calculations

Question 3d

Marks: 1

d)

The ionic product of water is 2.916 x 10^-14mol² dm^-6 at 313 K. What is the pH of water at this temperature?

[1]

Key Concepts

Acid-Base Calculations
The Ionic Product of Water

Question 4a

Marks: 2

a)

State one advantage and one disadvantage of using a pH meter instead of universal indicator to measure pH.

[2]

Key Concepts

pH Meters & Universal Indicator

Question 4b

Marks: 2

b)

State the name and formula of a strong alkali and a weak alkali.

[2]

Key Concepts

Strong & Weak Acids & Bases
Making Salts

Question 4c

Marks: 1

c)

State the meaning of the term dissociation as applied to acids and bases

Key Concepts

Strong & Weak Acids & Bases

Question 4d

Marks: 2

d)

Write equations for the dissociation of:

Nitric acid, HNO₃: ...................................

Methanoic acid, HCOOH: ............................

[2]

Key Concepts

Strong & Weak Acids & Bases

Question 4e

Marks: 1

e)

Identify the formula of the weakest conjugate base produced in the two acids in part d).

[1]

Key Concepts

Conjugate Pairs & Acid-Base Strength

Question 5a

Marks: 2

a)

Explain the difference between the terms strong acid and weak acid.

[2]

Key Concepts

Comparing Strong & Weak Acids

Question 5b

Marks: 2

b)

Other than measuring the pH, describe how you could distinguish between dilute solutions of the same concentration of hydrochloric acid and ethanoic acid.

[2]

Key Concepts

Comparing Strong & Weak Acids

Question 5c

Marks: 1

c)

A solution of 2.00 mol dm^-3 hydrochloric acid was added to marble chips and the volume of carbon dioxide recorded. A graph of the result is shown below:

On the same graph, sketch the result of repeating the experiment with 2.00 mol dm^-3ethanoic acid.

[1]

Key Concepts

Comparing Strong & Weak Acids
Rate of Reaction

Question 5d

Marks: 1

d)

The same experiment in part c) can be carried out by measuring how the mass of the reaction flask changes with time.

Sketch a graph of the expected result.

[1]

Key Concepts

Rate of Reaction
Comparing Strong & Weak Acids

DP IB Chemistry: SL

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