In a titration, 20.00 cm320.00\text{ cm}^320.00 cm3 of nitric acid (HNO3\text{HNO}_3HNO3) reacted with 24.00 cm324.00\text{ cm}^324.00 cm3 of 0.0500 mol/dm30.0500\text{ mol/dm}^30.0500 mol/dm3 barium hydroxide solution (Ba(OH)2\text{Ba(OH)}_2Ba(OH)2).
The equation for the reaction is:
2HNO3(aq)+Ba(OH)2(aq)→Ba(NO3)2(aq)+2H2O(l) 2\text{HNO}_3(\text{aq}) + \text{Ba(OH)}_2(\text{aq}) \rightarrow \text{Ba(NO}_3)_2(\text{aq}) + 2\text{H}_2\text{O(l)} 2HNO3(aq)+Ba(OH)2(aq)→Ba(NO3)2(aq)+2H2O(l)Calculate the concentration of the nitric acid in mol/dm3\text{mol/dm}^3mol/dm3.
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.