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
481–490 of 991
Question 481
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 482
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 483
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 484
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 485
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 486
2 marks · Normal
Answer and see the solution →Calculate the number of moles of potassium nitrate, KNO₃, in 25 cm³ of a solution with concentration 0.40 mol/dm³.
Question 487
4 marks · Normal
Answer and see the solution →A reaction between barium chloride and sodium sulfate is shown by the equation:
(a)[2 marks]Calculate the number of moles of Na₂SO₄ in 40 cm³ of solution with concentration 0.10 mol/dm³.
(b)[2 marks]Use the balanced equation to determine the number of moles of BaCl₂ that react with this amount of Na₂SO₄.
Question 488
3 marks · Normal
Answer and see the solution →What mass of magnesium sulfate, MgSO₄, is produced when 25 cm³ of 0.50 mol/dm³ sulfuric acid, H₂SO₄, reacts with excess magnesium oxide, MgO?
(Ar: Mg = 24, S = 32, O = 16)
Question 489
3 marks · Normal
Answer and see the solution →A student dissolves 0.015 mol of silver nitrate in 100 cm³ of water.
Explain how to work out the concentration of this solution in mol/dm³. Show your calculation.
Question 490
4 marks · Normal
Answer and see the solution →A student carries out a reaction between sodium hydroxide and hydrochloric acid:
Results table Experiment Volume of NaOH (cm³) Concentration of NaOH (mol/dm³) 1 20 0.25 2 15 0.25 3 25 0.50 (a)[2 marks]For experiment 2, calculate the number of moles of NaOH used.
(b)[2 marks]Using the equation, state the number of moles of HCl needed to react with the NaOH in experiment 2 and explain your answer.