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 sulfuric acid are ..
  • A.   magnesium sulfate and water
  • B.   magnesium sulfate and hydrogen
  • C.   magnesium sulfide and water
  • D.   magnesium sulfide and hydrogen
3. Which of the following statements about pH is correct?
  • A.   The lower the concentration of hydroxide ions in a solution the higher the pH
  • B.   The pH decreases when calcium oxide is added to dilute hydrochloric acid
  • C.   The higher the concentration of hydrogen ions in a solution the lower the pH
  • D.   Acidic solutions have a pH value above 7
4. Sulfuric acid is a strong acid. A strong acid is one which..
  • A.   is completely ionised in aqueous solution
  • B.   is partially ionised in aqueous solution
  • C.   contains a large amount of acid dissolved in water
  • D.   contains a small amount of acid dissolved in water
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 universal indicator red

6. Acids form salts. Select the row that correctly states the type of salt formed from each acid.

  Hydrochloric acid Sulfuric acid Nitric acid
A chlorate sulfide nitride
B chlorate sulfate nitrate
C chloride sulfate nitride
D chloride sulfate nitrate

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