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
211–220 of 423 · Normal
Question 211
1 mark · Normal
Answer and check →Which of the following shows the correct mass of sodium chloride produced when 0.020 mol of hydrochloric acid, HCl, reacts with excess sodium hydroxide, NaOH? (Ar: Na = 23, Cl = 35.5)
- A.0.585 g
- B.1.17 g
- C.2.34 g
- D.0.2925 g
Question 212
2 marks · Normal
Answer and see the solution →Calculate the number of moles of copper(II) sulfate in 200 cm³ of solution with concentration 0.050 mol/dm³.
Question 213
4 marks · Normal
Answer and see the solution →Potassium permanganate reacts with iron(II) sulfate as shown:
(a)[2 marks]Calculate the number of moles of FeSO₄ in 50 cm³ of 0.20 mol/dm³ solution.
(b)[2 marks]Use the equation to find the number of moles of KMnO₄ needed to react with this amount of FeSO₄.
Question 214
2 marks · Normal
Answer and see the solution →A student titrates 25.0 cm³ of potassium hydroxide solution of unknown concentration with 0.150 mol/dm³ hydrochloric acid. The average volume of acid required to neutralise the alkali is 18.0 cm³. Calculate the number of moles of hydrochloric acid ( ) used in the reaction.
Question 215
4 marks · Normal
Answer and see the solution →Ethanoic acid ( ) reacts with sodium hydroxide ( ) according to the equation:
A student titrates 25.0 cm³ of 0.200 mol/dm³ sodium hydroxide with ethanoic acid. On average, 21.0 cm³ of ethanoic acid is needed to neutralise the alkali.
(a)[1 mark]State the ratio in which sodium hydroxide reacts with ethanoic acid.
(b)[1 mark]Calculate the number of moles of sodium hydroxide present in 25.0 cm³.
(c)[1 mark]Calculate the number of moles of ethanoic acid used in the reaction.
(d)[1 mark]Calculate the concentration of the ethanoic acid.
Question 216
3 marks · Normal
Answer and see the solution →In a titration, 25.0 cm³ of sulphuric acid ( ) of unknown concentration is neutralised by 32.5 cm³ of 0.150 mol/dm³ potassium hydroxide ( ). The balanced chemical equation is:
Calculate the concentration of the sulphuric acid.
Question 217
4 marks · Normal
Answer and see the solution →A table shows the results from a titration between lithium hydroxide ( ) and hydrochloric acid ( ).
Titration Results Volume of LiOH (cm³) Concentration of LiOH (mol/dm³) Volume of HCl (cm³) Concentration of HCl (mol/dm³) 25.0 0.100 20.0 ? (a)[1 mark]Write the balanced chemical equation for this reaction.
(b)[1 mark]Calculate the number of moles of LiOH used.
(c)[1 mark]Using the chemical equation, state the number of moles of HCl that reacted.
(d)[1 mark]Calculate the concentration of the HCl solution.
Question 218
1 mark · Normal
Answer and check →Which step should you do first to solve for the unknown concentration in a standard titration calculation?
- A.Calculate the number of moles of the standard solution used
- B.Write the ionic equation for the reaction
- C.Multiply the concentrations of both solutions together
- D.Estimate the endpoint by eye only
Question 219
2 marks · Normal
Answer and see the solution →During a titration experiment, 22.5 cm³ of 0.250 mol/dm³ potassium hydroxide completely neutralises 27.0 cm³ of a sulfuric acid solution. Calculate the number of moles of potassium hydroxide used in the reaction.
Question 220
4 marks · Normal
Answer and see the solution →A sample of nitric acid ( ) reacts with sodium carbonate ( ) solution. The balanced equation is:
A student titrates 25.0 cm³ of 0.150 mol/dm³ sodium carbonate. On average, 36.0 cm³ of nitric acid is required to completely react.
(a)[1 mark]According to the equation, what is the ratio of moles of nitric acid to moles of sodium carbonate required?
(b)[1 mark]Calculate the number of moles of sodium carbonate used.
(c)[1 mark]Determine the number of moles of nitric acid required to react completely.
(d)[1 mark]Calculate the concentration of nitric acid in mol/dm³.