Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Inorganic Chemistry
869 practice questions
Topics covered
- The Alkali Metals85 practice questions
- The Halogens86 practice questions
- Gases in the Atmosphere86 practice questions
- Reactivity Series163 practice questions
- Extraction and Uses of Metals128 practice questions
- Acids, Alkalis and Titrations83 practice questions
- Acids, Bases and Salt Preparations156 practice questions
- Chemical Tests68 practice questions
Practice questions
361–370 of 374 · Normal
Question 361
4 marks · Normal
Answer and see the solution →(a)[2 marks]Name the compounds formed when silver nitrate is added to solutions containing (i) chloride, (ii) bromide, and (iii) iodide ions.
(b)[2 marks]Give the colour of each compound formed in part (a).
Question 362
2 marks · Normal
Answer and see the solution →State the names and colours of the precipitates formed when silver nitrate is added to (a) a solution containing bromide ions and (b) a solution containing iodide ions, after acidification with nitric acid.
Question 363
4 marks · Normal
Answer and see the solution →(a)[3 marks]Describe the steps you would take to test a sample for iodide ions using silver nitrate. Include all reagents added and any important precautions.
(b)[1 mark]What result would indicate that iodide ions are present?
Question 364
3 marks · Normal
Answer and see the solution →A student tests three unknown solutions by first adding dilute nitric acid and then silver nitrate solution. The results are:
Observations for unknown solutions after addition of silver nitrate Solution Observation A white precipitate B cream precipitate C no visible change Question 365
6 marks · Normal
Answer and see the solution →A student is given two separate white solids, labelled X and Y. X is known to be either sodium carbonate or ammonium chloride. Y is a mixture of calcium carbonate and ammonium chloride.
(a)Describe a test to identify which solid, X or Y, contains the carbonate ion. Calculate the minimum volume of 1.0 mol/dm³ hydrochloric acid required to completely react with 0.05 mol of carbonate present in one of the solids. Show your working.
(i)[1 mark]State what you would observe when dilute hydrochloric acid is added to a carbonate.
(ii)[1 mark]Write the ionic equation for the reaction of a carbonate ion with an acid.
(iii)[1 mark]Calculate the minimum volume (in cm³) of 1.0 mol/dm³ hydrochloric acid required to react completely with 0.05 mol of carbonate ion. (Assume carbonate is CO₃²⁻.)
(b)Solid Y is warmed with sodium hydroxide solution. Ammonia gas is produced.
Describe the test and give a calculation to show how many moles of ammonium ions would be present if 672 cm³ of ammonia gas is collected at room temperature and pressure. (1 mol of gas occupies 24,000 cm³ at r.t.p.)
(i)[1 mark]Describe how to test for ammonia gas.
(ii)[1 mark]Calculate the number of moles of ammonia gas in 672 cm³ at r.t.p.
(iii)[1 mark]Write the ionic equation for the reaction of ammonium ions with hydroxide ions.
Question 366
6 marks · Normal
Answer and see the solution →A student needs to check if water and carbonate ions are present in two different solutions. The first solution is labelled A (clear, colourless liquid). The second is labelled B (pale green solution).
(a)[2 marks]Describe how the student could test solution A to check if it is pure water. Explain the result that would show if it is not pure.
(b)[2 marks]The student adds a white powder to solution B and observes effervescence. The gas produced is bubbled through limewater which turns cloudy.
Explain what ions are present in the white powder and write the ionic equation for the reaction.
(c)[2 marks]The student wishes to know if any ammonium ions are present in the white powder. Describe a test for ammonium ions and explain how the result confirms their presence.
Question 367
6 marks · Normal
Answer and see the solution →A student tests an unknown powder. To show if the powder contains water and carbonate ions, the following experiments are carried out.
(a)[2 marks]Describe the chemical test used to show if the powder contains water.
(b)A sample of the powder is added to dilute acid and gas is released. The gas is bubbled through limewater, which becomes cloudy.
(i)[1 mark]Identify the ion present responsible for the release of this gas.
(ii)[2 marks]Write the ionic equation for the reaction between this ion and dilute acid.
(iii)[1 mark]Suggest a physical test to confirm if the water in the sample is pure.
Question 368
8 marks · Normal
Answer and see the solution →This question is about the properties of alkali metals and halogens.
(a)[2 marks]State the colour and physical state at room temperature for sodium and iodine.
(b)[2 marks]Describe how you would distinguish between a sample of potassium metal and a sample of lithium metal using their observable physical properties.
(c)[2 marks]Chlorine and sodium both have coloured vapours or solutions. Explain how the colour of chlorine gas compares with that of a solution containing iodine.
(d)[2 marks]State the trend in colour observed down Group 1 and down Group 7 elements.
Question 369
8 marks · Normal
Answer and see the solution →This question concerns the reactions of alkali metals and halogens.
(a)[2 marks]Describe what you would observe when a small piece of sodium is added to water. Give the word equation for the reaction.
(b)[2 marks]Compare the observations when potassium is added to water with those for sodium.
(c)[2 marks]State what you would observe when chlorine reacts with heated iron filings. Write the balanced chemical equation for the reaction.
(d)[2 marks]A solution contains sodium chloride and potassium iodide. Describe how you could use chlorine water to show a displacement reaction occurs, stating your observations.
Question 370
8 marks · Normal
Answer and see the solution →This question is about electronically explaining group reactivity and redox displacement.
(a)[3 marks]Explain why potassium is more reactive than sodium, referring to electronic structure.
(b)[3 marks]The reaction between chlorine and iodide ions is a redox displacement. Write the ionic equation for this reaction and state which substance is oxidised and which is reduced.
(c)[2 marks]Using electronic configurations, explain why chlorine is able to displace iodine from a solution of potassium iodide.