Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
Acids, Bases and Salt Preparations
156 practice questions
Topics covered
- Reactions of acids18 practice questions
- Reacting acids with bases19 practice questions
- Reacting acids with carbonates19 practice questions
- Salt preparations19 practice questions
- Making soluble salts (except sodium, potassium and ammonium salts)19 practice questions
- Making sodium, potassium and ammonium salts18 practice questions
- Making insoluble salts19 practice questions
- Theories of acids and bases19 practice questions
Practice questions
151–156 of 156
Question 151
5 marks · Easy
Answer and see the solution →This question is about the reactions of acids with different substances.
(a)[1 mark]State the general word equation for the reaction between a metal and an acid.
(b)[1 mark]Write a balanced symbol equation for the reaction between magnesium and dilute sulfuric acid.
(c)[1 mark]State the general word equation for the reaction between a metal oxide and an acid.
(d)[2 marks]Name the salt and the other product formed when copper(II) oxide reacts with dilute hydrochloric acid.
Question 152
5 marks · Easy
Answer and see the solution →This question is about preparing soluble salts using different methods.
(a)[1 mark]State why it is necessary to use an excess of the solid when preparing copper(II) sulfate from copper(II) oxide and sulfuric acid.
(b)[1 mark]Give one reason why you do not use the same 'excess solid' method for making sodium sulfate using sodium hydroxide and sulfuric acid.
(c)[1 mark]Give the name of the technique used instead to make sodium sulfate from sodium hydroxide and sulfuric acid.
(d)[2 marks]Explain briefly how you know when to stop adding acid during the preparation of sodium sulfate by this technique.
Question 153
5 marks · Easy
Answer and see the solution →This question is about the formation of crystals when preparing soluble salts.
(a)[2 marks]Explain why crystallisation is used instead of evaporating to dryness when making hydrated copper(II) sulfate crystals.
(b)[3 marks]Describe, in order, the steps taken after completing a titration to obtain pure sodium sulfate crystals from sodium hydroxide and sulfuric acid.
Question 154
5 marks · Easy
Answer and see the solution →This question is about preparing soluble salts and writing chemical equations for their formation.
(a)[2 marks]Write the balanced chemical equation for the reaction used to prepare hydrated magnesium sulfate crystals using magnesium carbonate and dilute sulfuric acid.
(b)[1 mark]A student wants to prepare pure sodium chloride crystals from sodium hydroxide and hydrochloric acid. Write the balanced chemical equation for this reaction.
(c)[1 mark]State one key difference between the methods used for preparing magnesium sulfate crystals and sodium chloride crystals in the laboratory.
(d)[1 mark]Calculate the mass of sodium chloride produced when 0.100 mol of hydrochloric acid reacts completely with sodium hydroxide. (Relative formula mass, NaCl = 58.5)
Question 155
6 marks · Normal
Answer and see the solution →(a)[1 mark]State the general word equation for the reaction between an acid and a carbonate.
(b)[1 mark]A student reacts magnesium carbonate with dilute hydrochloric acid. Name the gas that is produced in this reaction.
(c)[2 marks]Ammonium carbonate is one example of a soluble carbonate. Using your knowledge of solubility rules, name two other types of carbonates that are also soluble in water.
(d)[2 marks]Give a reason, using solubility rules, why lead(II) carbonate is not a suitable choice to make a soluble salt by the reaction with an acid.
Question 156
6 marks · Normal
Answer and see the solution →(a)[2 marks]Write a balanced chemical equation for the reaction between sodium carbonate and dilute nitric acid.
(b)[4 marks]Describe how you would prepare a pure sample of sodium nitrate using the reaction in part a. Include the main steps and explain how you would separate and obtain the pure salt.