Syllabus Edition

First teaching 2014

Last exams 2024

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More About Acids (DP IB Chemistry: SL)

Exam Questions

2 hours44 questions
1a1 mark

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

1b2 marks

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

1c
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1 mark

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.

1d1 mark

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

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2a1 mark

State the relationship between pH and hydrogen ion concentration.

2b
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1 mark

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

2c
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1 mark

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

2d1 mark

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

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3a1 mark

State what is meant by the ionic product of water.

3b
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1 mark

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

3c
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1 mark

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

3d
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1 mark

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

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4a
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2 marks

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

4b2 marks

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

4c1 mark

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

4d2 marks
Write equations for the dissociation of:

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

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

4e1 mark

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

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5a2 marks

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

5b2 marks

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

5c1 mark

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:


8-2-ib-sl-sq-easy-q5c-question

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

5d1 mark

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.

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1a2 marks

The equilibrium constant for the first dissociation of formic acid is 1.8 x 10-4 mol dm-3.

State, with a reason, the strength of formic acid.

1b1 mark

Outline one laboratory method used to distinguish between equimolar solutions of formic acid and hydrochloric acid, giving the expected observations.

1c2 marks

Formic acid has the chemical formula HCOOH. Identify the conjugate base of formic acid and state whether it is a weak or strong conjugate base.

1d2 marks

Draw the structure of formic acid and give its systematic IUPAC name.

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2a2 marks

The pH of an aqueous solution of salicylic acid at 298 K is 3.85. Determine the concentration of hydroxide ions in the solution, using Section 2 of the Data booklet.

2b3 marks

A and B are two solutions of the same concentrations that have pH values of 3 and 6 respectively. 

i)
Identify which is the stronger acid and calculate the concentration of hydrogen ions in each solution.

ii)
Calculate the ratio of the hydrogen ion concentrations in both A and B.
2c3 marks

The variation of conductivity and concentration of a strong and weak monoprotic acid are shown in Figure 1.

Identify the strong and weak acid from the information given and justify your choices.

VcCyqkCr_1

2d1 mark

For acid 1 and acid 2 in part (c) compare the volume of 0.2 mol dm-3 NaOH required to neutralise 20 cm3 of 0.1 mol dm-3 solutions of the acids.

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3a3 marks

The concentrations of solutions of weak acids can be determined by titration against standard solutions of alkalis, such as sodium hydroxide.

i)
Explain what is meant by the term standard solution.

ii)
State the name of the indicator which should be used for this titration and what would be observed at the equivalence point of the reaction if the sodium hydroxide is placed in the burette.
3b3 marks

A solution of 25.0 cm3 ethanoic acid was titrated against 0.150 mol dm-3 NaOH (aq) and it was found that 22.35 cm3 of the NaOH was needed for complete neutralisation.

Write an equation for the reaction and determine the concentration of the ethanoic acid.

3c2 marks

A solution of 0.1 mol dm-3 ammonia has a pH of approximately 11. Predict how the pH value of 0.1 mol dm-3 sodium hydroxide solution would compare and calculate its value.

3d2 marks

Write an equation for the reaction between ammonia and water and use it to classify each product as a Brønsted–Lowry acid or base.

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4a2 marks

Glycolic acid, C2H4O3, is an organic acid sometimes used to remove limescale, CaCO3, from electric kettles and coffee machines.

Predict, with a reason, a difference in the reaction between the same concentration of sulfuric acid and glycolic acid with samples of calcium carbonate.

4b3 marks

Another acid that is sometimes used to descale kettles is sulfamic acid, NH2SO3H. Sulfamic is classed as a strong monoprotic acid.

i)
Explain the meaning of the term strong monoprotic acid.

ii)

Calculate the pH of a 0.136 mol dm-3 solution of sulfamic acid and determine the concentration of hydroxide ions in the solution at 298 K.

4c2 marks

A solution of hydrochloric acid has a pH of 1 and a solution of carbonic acid has a pH of 5. Determine the ratio of hydrogen ion concentrations of hydrochloric acid to carbonic acid.

4d4 marks

Outline two ways, apart from using pH, which could allow you to distinguish between two solutions of carbonic acid and hydrochloric acid that have the same concentration.

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5a1 mark

Four solutions of acids with identical concentrations are prepared. The equilibrium constants of these acids are given in Table 1.

Table 1

Acid

Kc mol dm-3 at 298 K

HCN

4.9 x 10-10

HF

6.8 x 10-4

CH3COOH

1.7 x 10-5

HCl

1.3 x 106

Write down the acid dissociation equation for HCN.

5b2 marks

Use the information in part (a) to complete this question.

i)
Write down the list of acids in part (a) in order of decreasing pH.

ii)
Write down the list of acids in order of increasing concentration of molecules of the acid present in the solution.
5c2 marks

State the name and formula of all the chemical species present in the solution of CH3COOH.

5d1 mark

Write the name and formula of the conjugate base of HF.

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1a
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4 marks

A solution of hydrochloric acid of concentration 0.001 mol dm-3 has a pH value of 3. Suggest, giving a reason, the pH of the following solutions of acids:

i)
0.01 mol dm-3 hydrochloric acid
[2]

ii)
0.01 mol dm-3 ethanoic acid
[2]
1b
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1 mark

A solution of 0.01 mol dm-3 ethanoic acid has a concentration of hydrogen ion of 1 x 10-4 mol dm-3.  Determine the percentage of ethanoic acid molecules that have dissociated.

1c1 mark

Two separate titrations are carried out using 25.00 cm3 of 0.01 mol dm-3 solutions of hydrochloric acid followed by ethanoic acid, against 0.01 mol dm-3 sodium hydroxide. 

State what difference(s) would be observed in the two titrations.  

1d
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2 marks

Suggest a suitable indicator for the titration of hydrochloric acid and sodium hydroxide in part c), and state the colour changes observed.

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2a3 marks

Show how the ionic product for water is derived from the dissociation of water and give it units.

2b
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1 mark

Determine the pH of 0.001 mol dm-3 sodium hydroxide.

2c4 marks

Suggest, with a reason, how the magnitude of Kw changes with increasing temperature.

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3a1 mark

Malonic acid is a weak dibasic carboxylic acid with the formula C3H4O4. Draw the displayed structure of malonic acid.

3b2 marks

Suggest, with a reason, which of the two acids, ethanoic or malonic, has a higher pH?

3c1 mark

Apart from testing the pH, suggest how equimolar solutions of malonic acid and ethanoic acid may be distinguished.

3d2 marks

Write the formulas of two conjugate bases that can be formed from malonic acid.

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4a2 marks

Marble chips are added separately to solutions of the same concentration of ethanoic acid and hydrochloric acid. State one similarity and one difference you would expect to observe in the reactions.

4b1 mark

Write an equation for the reaction between marble chips and ethanoic acid.

4c
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3 marks

Determine the volume, in cm3, of 2.25 mol dm-3 ethanoic acid needed to completely react with 1.50 g of marble chips. 

4d
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3 marks

Determine the volume of CO2, in cm3, produced at 273 K and 101 kPa in part c).

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