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Chemistry CIE iGCSE:
Acids, Bases + Salts 1

Page 1



1. Rain water is weakly acidic because it contains dissolved carbon dioxide. Which of these is a possible pH for rain water?

2. The products of the reaction between magnesium and hydrochloric acid are ...
  • A.   magnesium chloride and water
  • B.   magnesium chloride and hydrogen
  • C.   magnesium chlorate and water
  • D.   magnesium chlorate and hydrogen
3. Four solutions with different pH values were tested with universal indicator.

Which row shows the colour of each solution after the indicator was added?

  pH 9 pH 1 pH7 pH6
A purple red yellow orange
B red yellow green blue
C blue red green yellow
D blue green yellow orange
4. Slaked lime (calcium hydroxide) is used to neutralize acidic soils.

Farmer using lime to neutralise soil
Peter Turner | CC-BY-SA 2.0

Which ion is responsible for neutralizing the acid in the soil?
  • A.   Ca2+
  • B.   H+
  • C.   OH-
  • D.   O2-
5. Which is NOT a typical characteristic of acids?
  • A.   They react with metal oxides producing hydrogen
  • B.   They react with carbonates producing carbon dioxide
  • C.   They react with alkalis producing water
  • D.   They turn blue litmus paper red

6. The pH values of four aqueous solutions are:

Solution pH
P 13
Q 7
R 2
S 9

Which of these solutions are alkaline?

  • A.   R only
  • B.   R and Q only
  • C.   Q, S and P only
  • D.   S and P only

A student prepared a sample of hydrated copper(II)sulfate crystals by reacting excess copper(II)carbonate with dilute sulfuric acid.

copper sulfate crystals
Crystal Titan | CC 4.0

7. The equation for this reaction with the correct state symbols is ..
  • A.  CuCO3(s) + H2SO4(l)  CuSO4(l) + H2O(l) + CO2(g)
  • B.  CuCO3(s) + H2SO4(aq)  CuSO4(aq) + H2O(l) + CO2(g)
  • C.  CuCO3(s) + H2SO4(l)  CuSO4(aq) + H2O(l) + CO2(g)
  • D.  CuCO3(aq) + H2SO4(aq)  CuSO4(aq) + H2O(l) + CO2(g)
8. How would the student know when she had added an excess of copper(II)carbonate?
  • A.   the solution would turn blue in colour
  • B.   the temperature would rise
  • C.   effervescence would stop and solid would remain in the mixture
  • D.   all the solid would disappear

9. What techniques would the student use to:

(a) separate the excess copper(II)carbonate from the mixture?
(b) obtain hydrated copper(II)sulfate crystals from the solution?

  Separate excess copper(II) carbonate Obtain hydrated copper(II)sulfate crystals
A filtration crystallisation
B evaporation distillation
C filtration distillation
D evaporation crystallisation
10. Why was excess copper(II)carbonate used in the salt preparation?
  • A.   To ensure that a reaction takes place
  • B.   To speed up the reaction
  • C.   To allow the solid to be separated from the solution
  • D.   To ensure that all the acid is used up