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
91–100 of 136 · Hard
Question 91
7 marks · Hard
Answer and see the solution →The metal iron is widely used in construction and manufacturing. Iron is typically extracted from its ore, haematite, which contains iron(III) oxide.
(a)[1 mark]State what is meant by the term "ore".
(b)[2 marks]Iron is found below carbon in the reactivity series.
Explain why carbon can be used to extract iron from its oxide, but cannot be used to extract aluminium from aluminium oxide.
(c)[2 marks]Write a balanced chemical equation for the reduction of iron(III) oxide with carbon monoxide.
(d)[2 marks]Suggest one economic reason why extraction by heating with carbon is preferred for some metals rather than extraction by electrolysis.
Question 92
2 marks · Hard
Answer and see the solution →State the colours that phenolphthalein and methyl orange turn in a strongly alkaline solution.
Question 93
5 marks · Hard
Answer and see the solution →An unknown solution is tested with universal indicator. The indicator turns blue-green and the estimated pH is 8.
(a)[2 marks]Use the pH scale to classify the solution as strongly acidic, weakly acidic, neutral, weakly alkaline, or strongly alkaline. Give a reason for your answer.
(b)[1 mark]State what the pH value tells you about the concentration of hydrogen ions compared to a solution of pH 7.
(c)[2 marks]Describe how you would use universal indicator to estimate the pH of an aqueous solution. Include what you would observe and what you would compare it to.
Question 94
2 marks · Hard
Answer and see the solution →Explain how adding an acid to an alkaline solution changes its pH. State what happens to the indicator colour if universal indicator is used throughout.
Question 95
2 marks · Hard
Answer and see the solution →State the colours shown by phenolphthalein in (i) a strongly acidic solution, and (ii) a strongly alkaline solution.
Question 96
5 marks · Hard
Answer and see the solution →For each pH value below, state whether the solution is strongly acidic, weakly acidic, neutral, weakly alkaline, or strongly alkaline.
(a)[1 mark]pH = 2
(b)[1 mark]pH = 5
(c)[1 mark]pH = 7
(d)[1 mark]pH = 9
(e)[1 mark]pH = 12
Question 97
2 marks · Hard
Answer and see the solution →Describe how you would use universal indicator paper to measure the pH of a solution as accurately as the method allows.
Question 98
2 marks · Hard
Answer and see the solution →State the name and the full chemical formula of the ion that is present in all acidic solutions and causes acidity.
Question 99
5 marks · Hard
Answer and see the solution →The following table shows two acids and their reactions in water.
Acid Equation in water Acid A Acid B (a)[1 mark]For Acid A, explain what the presence of H^+ ions in solution tells you about the nature of the solution.
(b)[1 mark]For Acid B, how many moles of H^+ ions are formed from 1 mole of HB_2?
(c)[2 marks]Both Acid A and Acid B are added separately to water to make solutions.
Describe in terms of ions what occurs in each solution and which property they share.
(d)[1 mark]Explain, using one example from above, what is meant by the 'replaceable hydrogen' in acids.
Question 100
2 marks · Hard
Answer and see the solution →Name one metal compound (other than ammonia or sodium hydroxide) that makes water alkaline and write a balanced equation to show the formation of hydroxide ions in this solution.