Solution P contains lead nitrate. Solution Q contains both ammonium sulfate and sodium chloride. A precipitate forms when P and Q are mixed.
Statement 1: Pb2+(aq)+SO42−(aq)→PbSO4(s)\mathrm{Pb^{2+}(aq) + SO_{4}^{2-}(aq) \rightarrow PbSO_{4}(s)}Pb2+(aq)+SO42−(aq)→PbSO4(s)
Statement 2: Pb2+(aq)+2Cl−(aq)→PbCl2(s)\mathrm{Pb^{2+}(aq) + 2Cl^{-}(aq) \rightarrow PbCl_{2}(s)}Pb2+(aq)+2Cl−(aq)→PbCl2(s)
Statement 3: NH4+(aq)+NO3−(aq)→NH4NO3(s)\mathrm{NH_{4}^{+}(aq) + NO_{3}^{-}(aq) \rightarrow NH_{4}NO_{3}(s)}NH4+(aq)+NO3−(aq)→NH4NO3(s)
Statement 4: Na+(aq)+NO3−(aq)→NaNO3(s)\mathrm{Na^{+}(aq) + NO_{3}^{-}(aq) \rightarrow NaNO_{3}(s)}Na+(aq)+NO3−(aq)→NaNO3(s)
Which ionic equations represent the formation of a precipitate in this mixture?
1 only
1 and 2 only
1, 2 and 3 only
2 and 4 only
44 exam-style questions on Edexcel GCSE Chemistry 4.1 Acids, covering 4.1.1 Acids, alkalis and the pH scale, 4.1.2 Hydrogen ion concentration and pH, 4.1.3 Dilute and concentrated, weak and strong acids, 4.1.4 Bases, alkalis and the reactions of acids, 4.1.5 Chemical tests for hydrogen and carbon dioxide, 4.1.6 Neutralisation as a reaction of acids with bases, 4.1.7 Preparing soluble salts, and 4.1.8 Solubility rules and preparing insoluble salts. Each one has a worked solution and a mark scheme showing where the marks go.