This question is about acids and bases.
Give the chemical formula of the ion that is responsible for making an aqueous solution acidic.
A student performs a titration using sodium hydroxide solution and dilute sulfuric acid.
The chemical equation for this neutralisation reaction is:
2NaOH(aq)+H2SO4(aq)→Na2SO4(aq)+2H2O(l) 2\text{NaOH}(\text{aq}) + \text{H}_2\text{SO}_4(\text{aq}) \rightarrow \text{Na}_2\text{SO}_4(\text{aq}) + 2\text{H}_2\text{O}(\text{l}) 2NaOH(aq)+H2SO4(aq)→Na2SO4(aq)+2H2O(l)During the titration, 20.0 cm320.0\text{ cm}^320.0 cm3 of 0.150 mol/dm30.150\text{ mol/dm}^30.150 mol/dm3 sodium hydroxide solution is completely neutralised by 18.5 cm318.5\text{ cm}^318.5 cm3 of sulfuric acid.
Calculate the concentration of the sulfuric acid in mol/dm3\text{mol/dm}^3mol/dm3. Give your final answer to 3 significant figures.
To find this, you should calculate:
An aqueous solution of nitric acid with pH 3.8\text{pH } 3.8pH 3.8 has a hydrogen ion concentration of 1.58×10−4 mol/dm31.58 \times 10^{-4}\text{ mol/dm}^31.58×10−4 mol/dm3.
What is the concentration of H+\text{H}^+H+ ions in a solution of nitric acid with pH 1.8\text{pH } 1.8pH 1.8?
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.