AQA GCSE Chemistry

Topic Questions

4.2 Reactions of Acids

11 mark

Calcium reacts with hydrochloric acid to form the salt, calcium chloride and another product. 

calcium  +   hydrochloric acid            →         calcium chloride  + ___________

What is the unknown product?

  • Water 

  • Oxygen

  • Hydrogen

  • Carbon dioxide 

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21 mark

Indicators are used during a titration to observe the end point. 

Different indicators turn different colours in acids and alkalis.

Which indicator displays the correct colour in each solution?

Indicator Colour in acid  Colour in alkali 
methyl orange red  yellow
universal indicator red  orange
litmus red  purple
phenolphthalein red  colourless 

  • Methyl orange

  • Universal indicator

  • Litmus

  • Phenolphthalein

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3
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1 mark

A solution of sulfuric acid with a pH of 4 has a hydrogen ion concentration of 1 x 10-4 mol/dm3.

Another acid has a hydrogen ion concentration of 1 x 10-6 mol/dm3.

What is the pH of this acid?

  • 2

  • 3

  • 5

  • 6

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4
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1 mark

A student carrying out a titration finds that a 25.0 cm3 solution of 0.500 mol/dm3 hydrochloric acid neutralises 35.0 cm3 of sodium hydroxide. 

The balanced symbol equation for the reaction is:

NaOH + HCl  →    NaCl  + H2O

What is the concentration of the sodium hydroxide?

  • 0.15 mol/dm3

  • 0.36 mol/dm3

  • 0.72 mol/dm3

  • 1.00 mol/dm3

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5
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1 mark

What is the ionic equation for neutralisation?

  • 2H(aq) + OH(aq)   →    H2O (l)

  • H(aq) + OH(aq)   →    H2O (aq)

  • H(aq) + OH(aq)   →    H2O (l)

  • 2H2 + O2    →       2H2O

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61 mark

A student making copper sulfate crystals used the method below. 

q6

Unreacted copper carbonate was left over as it had been added in excess.

What is the reason for adding it in excess and what would step 3 be of this method?

  Reason for adding excess copper carbonate Step 3 of method
A to produce a greater amount of salt crystals filtration
B to improve the colour intensity of the crystals crystallisation
C to ensure all the acid reacts filtration
D to increase the rate of reaction evaporation

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71 mark

A student added some sulfuric acid gradually to a solution of ammonia until it was in excess.

What happens to the pH during this reaction?

  pH of ammonia at start pH after addition of excess sulfuric acid 
A 11 7
B 7 13
C 11 2
D 3 8

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