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
331–340 of 374 · Normal
Question 331
4 marks · Normal
Answer and see the solution →The table below shows five example reactions. For each reaction, state which theory (Arrhenius, Bronsted-Lowry, or both) can be used to explain it, and give a reason for your choice.
Acid-base reactions for theory comparison Equation Theory (Arrhenius / Bronsted-Lowry / Both) Reason HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) HCl(g) + NH3(g) → NH4Cl(s) HNO3(aq) + NH3(aq) → NH4NO3(aq) H2O(l) + NH3(g) → NH4^+(aq) + OH^-(aq) NH4^+(aq) + OH^-(aq) → NH3(aq) + H2O(l) Question 332
1 mark · Normal
Answer and check →According to the Bronsted-Lowry theory, what is a base?
- A.A substance that donates a proton.
- B.A substance that accepts a proton.
- C.A substance that donates electrons.
- D.A substance that accepts electrons.
Question 333
2 marks · Normal
Answer and see the solution →Use the Bronsted-Lowry definition to identify the acid and base in the following reaction: \[ H_2SO_4(aq) + CuO(s) \rightarrow CuSO_4(aq) + H_2O(l) \] State which is the acid and which is the base.
Question 334
4 marks · Normal
Answer and see the solution →The hydroxonium ion, H_3O^+, plays a key role in acidbase reactions.
(a)[2 marks]Draw a dot-and-cross diagram to show the bonding in a hydroxonium ion, H_3O^+.
(b)[2 marks]Explain, in terms of proton transfer, how H_3O^+ is formed from HCl and H_2O.
Question 335
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 336
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.
Question 337
2 marks · Normal
Answer and see the solution →State the result of the test for ammonia gas using damp red litmus paper. Explain why this result occurs.
Question 338
4 marks · Normal
Answer and see the solution →A student is given an unknown liquid and asked to test for the presence and purity of water.
(a)[2 marks]Describe how the student could use anhydrous copper(II) sulfate to test for the presence of water in the liquid.
(b)[2 marks]Explain how the student could determine if the liquid is pure water.
Question 339
3 marks · Normal
Answer and see the solution →A sample of gas in a test-tube is suspected to be ammonia. A student tests this gas using damp red litmus paper. He repeats the test with chlorine gas for comparison.
(a)[1 mark]State the result when ammonia gas is tested with damp red litmus paper.
(b)[1 mark]State the result when chlorine gas is tested with damp red litmus paper.
(c)[1 mark]Explain how these tests can be used to identify ammonia gas in a mixture of alkaline and acidic gases.
Question 340
3 marks · Normal
Answer and see the solution →A student tests two samples, A and B, for water. Both samples turn white anhydrous copper(II) sulfate blue. When heated, sample A boils at 102°C and sample B boils at 100°C (at 1 atm pressure).
Explain, with reasons, which sample is pure water and which is not.