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4.2 Reactions of acids

4.2 Reactions of acids

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Question 27

Malonic acid is a white crystalline solid at room temperature.

a.

Calculate the mass of malonic acid (H2C3H2O4\text{H}_2\text{C}_3\text{H}_2\text{O}_4H2​C3​H2​O4​) needed to make 500 cm3500\text{ cm}^3500 cm3 of a solution with concentration 0.0450 mol/dm30.0450\text{ mol/dm}^30.0450 mol/dm3.

Relative formula mass (MrM_rMr​): H2C3H2O4=104\text{H}_2\text{C}_3\text{H}_2\text{O}_4 = 104H2​C3​H2​O4​=104

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b.

A student found that 20.0 cm320.0\text{ cm}^320.0 cm3 of a potassium hydroxide solution was neutralised by 16.80 cm316.80\text{ cm}^316.80 cm3 of the 0.0450 mol/dm30.0450\text{ mol/dm}^30.0450 mol/dm3 malonic acid solution.

The equation for the reaction is:

H2C3H2O4+2KOH→K2C3H2O4+2H2O \text{H}_2\text{C}_3\text{H}_2\text{O}_4 + 2\text{KOH} \rightarrow \text{K}_2\text{C}_3\text{H}_2\text{O}_4 + 2\text{H}_2\text{O} H2​C3​H2​O4​+2KOH→K2​C3​H2​O4​+2H2​O

Calculate the concentration of the potassium hydroxide solution in mol/dm3\text{mol/dm}^3mol/dm3.

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Markscheme

4.2 Reactions of acids Questions

  1. GCSE
  2. /Chemistry
  3. /4.2 Reactions of acids

40 exam-style questions on AQA GCSE Chemistry 4.2 Reactions of acids, covering 4.2.1 Reactions of acids with metals, 4.2.2 Neutralisation of acids and salt production, 4.2.3 Soluble salts, 4.2.4 The pH scale and neutralisation, 4.2.5 Titrations, and 4.2.6 Strong and weak acids (HT only). Each one has a worked solution and a mark scheme showing where the marks go.

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