Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Principles of Chemistry
991 practice questions
Topics covered
- States of Matter102 practice questions
- Elements, Compounds and Mixtures69 practice questions
- Atomic Structure108 practice questions
- The Periodic Table103 practice questions
- Chemical Formulae, Equations and Calculations Part 119 practice questions
- Chemical Formulae, Equations and Calculations Part 2144 practice questions
- Ionic Bonding143 practice questions
- Covalent Bonding68 practice questions
- Metallic Bonding19 practice questions
- Electrolysis198 practice questions
Practice questions
201–210 of 407 · Easy
Question 201
2 marks · Easy
Answer and see the solution →A student adds 50 cm³ of 0.20 mol/dm³ hydrochloric acid, HCl, to excess calcium carbonate, CaCO₃.
The equation is:
Explain, using calculations, how to find the mass of CaCO₃ that will react with the HCl. Include your method and final answer. (Ar: Ca = 40, C = 12, O = 16)
Question 202
3 marks · Easy
Answer and see the solution →A student prepares solutions of nitric acid with different concentrations. The table shows the volume and concentration of nitric acid used in each experiment.
Volume and concentration data for nitric acid solutions. Experiment Volume (cm³) Concentration (mol/dm³) 1 25 0.20 2 40 0.10 3 50 0.16 Calculate the number of moles of nitric acid in each experiment. Give your answers to two decimal places.
(a)[1 mark]Experiment 1:
(b)[1 mark]Experiment 2:
(c)[1 mark]Experiment 3:
Question 203
1 mark · Easy
Answer and see the solution →The balanced equation for the reaction between hydrochloric acid and sodium carbonate is:
If 0.04 mol of sodium carbonate reacts completely, how many moles of hydrochloric acid are required to react with it?
Question 204
3 marks · Easy
Answer and see the solution →Zinc sulfate can be made by reacting zinc oxide with sulfuric acid as follows:
(a)[1 mark]25 cm³ of 0.20 mol/dm³ sulfuric acid is used in the reaction. Calculate the number of moles of sulfuric acid used.
(b)[1 mark]How many moles of zinc sulfate could be formed from this amount of sulfuric acid?
(c)[1 mark]Calculate the maximum mass of zinc sulfate, ZnSO₄ (Mᵣ = 161), formed.
Question 205
2 marks · Easy
Answer and see the solution →Calculate the number of moles of potassium chloride, KCl, dissolved in 15 cm³ of solution with a concentration of 0.25 mol/dm³.
Question 206
1 mark · Easy
Answer and see the solution →State the first step you should always take when calculating the concentration of a solution using the three-step titration calculation method.
Question 207
3 marks · Easy
Answer and see the solution →A student is titrating 25.0 cm³ of sodium hydroxide solution with hydrochloric acid. The concentration of sodium hydroxide is 0.200 mol/dm³.
(a)[2 marks]Calculate the number of moles of sodium hydroxide in 25.0 cm³.
(b)[1 mark]State the equation you would use for this calculation.
(c)[0 marks]Give the unit for the concentration used in the calculation.
Question 208
2 marks · Easy
Answer and see the solution →The equation for the reaction is:
In a titration, 35.0 cm³ of 0.300 mol/dm³ potassium hydroxide are used. Calculate the number of moles of sulfuric acid that will react with this amount, using the equation.
Question 209
2 marks · Easy
Answer and see the solution →Explain, using the three-step titration calculation method, how you can find the concentration of an unknown acid after titrating it with a solution of known concentration.
Question 210
3 marks · Easy
Answer and see the solution →A student has the following titration results:
Titration Volume of NaOH (cm³) Concentration of NaOH (mol/dm³) 1 22.0 0.150 2 21.5 0.150 3 (repeat) 21.7 0.150 The student used 25.0 cm³ of hydrochloric acid of unknown concentration each time. Use the results to calculate the mean number of moles of sodium hydroxide used to neutralise the acid.