A water company tests a sample of river water for chloride ions and sulfate ions.
Silver nitrate solution is added to a sample of the water, acidified with dilute nitric acid. State the colour of the precipitate that forms if chloride ions are present.
The equation for the reaction of silver nitrate with sodium chloride is:
AgNO3(aq)+NaCl(aq)→AgCl(s)+NaNO3(aq)\mathrm{AgNO_{3}(aq)} + \mathrm{NaCl(aq)} \rightarrow \mathrm{AgCl(s)} + \mathrm{NaNO_{3}(aq)}AgNO3(aq)+NaCl(aq)→AgCl(s)+NaNO3(aq)
Identify the two spectator ions in this reaction.
Write the ionic equation for this reaction, including state symbols.
Sulfate ions are detected with barium chloride solution. The equation for the reaction with sodium sulfate is:
BaCl2(aq)+Na2SO4(aq)→BaSO4(s)+2NaCl(aq)\mathrm{BaCl_{2}(aq)} + \mathrm{Na_{2}SO_{4}(aq)} \rightarrow \mathrm{BaSO_{4}(s)} + \mathrm{2NaCl(aq)}BaCl2(aq)+Na2SO4(aq)→BaSO4(s)+2NaCl(aq)
Write the ionic equation for this reaction, including state symbols.
Explain why the ionic equation for the reaction of silver nitrate solution with potassium chloride solution is the same as the ionic equation in (b)(ii).
230 exam-style questions on Edexcel GCSE Chemistry 1.1 Formulae, equations and hazards, covering 1.1.1 Formulae, word and balanced equations, 1.1.2 Balanced ionic equations, and 1.1.3 Hazard symbols and risk in practical work. Each one has a worked solution and a mark scheme showing where the marks go.