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
351–360 of 374 · Normal
Question 351
2 marks · Normal
Answer and see the solution →Describe how you would test a solid sample to show that it contains carbonate ions (). State what you would observe if carbonate ions are present.
Question 352
2 marks · Normal
Answer and see the solution →State the substance you would add to a sample to test for carbonate ions, and describe what you would observe if carbonate ions are present.
Question 353
4 marks · Normal
Answer and see the solution →A student is given a white powder thought to contain carbonate ions.
(a)[1 mark]The student adds dilute hydrochloric acid to the powder.
State what the student should observe if carbonate ions are present.
(b)[1 mark]The student collects the gas given off and bubbles it through limewater. What result would confirm the gas is carbon dioxide?
(c)[2 marks]Write the ionic equation for the reaction between carbonate ions and hydrochloric acid.
Question 354
3 marks · Normal
Answer and see the solution →A student tests 0.30 g of potassium carbonate ([K\ce{K2CO3}) powder with excess dilute hydrochloric acid. All of the carbonate reacts.
(a)[1 mark]Write the chemical equation, including state symbols, for the reaction between potassium carbonate and hydrochloric acid.
(b)[1 mark]Calculate the number of moles of potassium carbonate in 0.30 g. (Relative formula mass, , of \ce{K2CO3} = 138.0.)
(c)[1 mark]Calculate the volume of carbon dioxide gas produced at room temperature and pressure (RTP), in cm. (1 mole of gas at RTP occupies 24 000 cm.)
Question 355
2 marks · Normal
Answer and see the solution →Describe the steps you would take to test a solution for the presence of chloride, bromide, and iodide ions using silver nitrate.
Question 356
4 marks · Normal
Answer and see the solution →(a)[1 mark]State the expected observation if chloride ions are present when silver nitrate solution is added after acidifying.
(b)[1 mark]State the expected observation if bromide ions are present when silver nitrate solution is added after acidifying.
(c)[1 mark]State the expected observation if iodide ions are present when silver nitrate solution is added after acidifying.
(d)[1 mark]A student tested a solution using dilute nitric acid and silver nitrate. The result was a cream precipitate. Which ion is present?
Question 357
3 marks · Normal
Answer and see the solution →Explain how you can distinguish between the precipitates formed when chloride, bromide or iodide ions react with silver nitrate. In your answer, refer to both the name and the colour of each precipitate.
Question 358
4 marks · Normal
Answer and see the solution →The table shows the results of silver nitrate tests on four unknown solutions after they were all acidified with dilute nitric acid.
Solution Observation with AgNO3 after acidifying P White precipitate Q Yellow precipitate R No precipitate S Cream precipitate For each solution, write the name and formula of the ion responsible for the observation. If there is no precipitate, state 'none'.
Question 359
1 mark · Normal
Answer and check →A solution is acidified with dilute nitric acid and then tested with silver nitrate. Which observation indicates the presence of bromide ions?
- A.A yellow precipitate forms.
- B.A white precipitate forms.
- C.A cream precipitate forms.
- D.No precipitate forms.
Question 360
2 marks · Normal
Answer and see the solution →State two reasons why nitric acid is used, and not hydrochloric acid, when testing for halide ions with silver nitrate.