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
21–30 of 66 · Normal
Question 21
1 mark · Normal
Answer and check →Which of the following is the balanced chemical equation for the reaction of zinc carbonate with hydrochloric acid?
- A.\ce{ZnCO3(s) + 2HCl(aq) -> ZnCl2(aq) + CO2(g) + H2O(l)}
- B.\ce{ZnCO3(s) + HCl(aq) -> ZnCl2(aq) + CO2(g)}
- C.\ce{ZnCO3(s) + 2HCl(aq) -> ZnCl2(aq) + CO2(g)}
- D.\ce{ZnCO3(s) + HCl(aq) -> ZnCl(aq) + CO2(g) + H2O(l)}
Question 22
2 marks · Normal
Answer and see the solution →Name the two products formed, apart from the salt, when a carbonate reacts with a dilute acid.
Question 23
4 marks · Normal
Answer and see the solution →(a)[2 marks]Write the ionic equation for the reaction between carbonate ions and hydrogen ions.
(b)[2 marks]Explain why water is formed in this reaction.
Question 24
3 marks · Normal
Answer and see the solution →A student adds powdered calcium carbonate to an excess of dilute nitric acid in a beaker. Bubbles of gas are observed.
State the chemical names of the three products formed in this reaction.
Question 25
2 marks · Normal
Answer and see the solution →State whether each of the following compounds is soluble or insoluble in water, according to the solubility rules:
(a)Lead(II) sulfate
(b)[1 mark]Potassium carbonate
(b)[1 mark]Question 26
3 marks · Normal
Answer and see the solution →A student is given a sample of calcium hydroxide and is told that calcium hydroxide is only slightly soluble in water. Using the solubility rules, calculate how many of the following compounds are soluble in water:
Compound Sodium nitrate Barium sulfate Potassium carbonate Calcium sulfate Ammonium chloride State the total number of compounds from the table that are soluble in water.
Question 27
1 mark · Normal
Answer and check →Which method is most suitable for preparing a pure, dry sample of potassium nitrate in the laboratory?
- A.Reacting dilute nitric acid with potassium hydroxide and crystallising from solution
- B.Reacting potassium carbonate with dilute hydrochloric acid and filtering the mixture
- C.Mixing potassium nitrate with water and filtering out the excess solid
- D.Reacting potassium nitrate with silver nitrate and collecting the precipitate
Question 28
4 marks · Normal
Answer and see the solution →Iron(II) sulfate can be made by reacting an acid with a suitable base in the laboratory.
(a)Name two reactants you could use to prepare iron(II) sulfate.
(b)[1 mark]Write the balanced chemical equation for this reaction.
(c)[3 marks]Describe the steps you would take to obtain pure iron(II) sulfate crystals from the reaction mixture.
Question 29
4 marks · Normal
Answer and see the solution →A student wants to prepare a pure, dry sample of barium sulfate in the laboratory. Barium sulfate is insoluble in water.
(a)[1 mark]Name two suitable soluble solutions that could be mixed to prepare barium sulfate.
(b)[2 marks]Describe the steps the student should follow to obtain pure, dry barium sulfate from the mixture after the reaction is complete.
(c)[1 mark]Explain why filtration is necessary in this method.
Question 30
3 marks · Normal
Answer and see the solution →Copper(II) sulfate can be made by adding excess copper(II) oxide to dilute sulfuric acid.
(a)[1 mark]Explain why an excess of copper(II) oxide is added during the preparation.
(b)[2 marks]Describe what the student should do after all the acid has reacted, to obtain dry copper(II) sulfate crystals.