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(a) Classify the following reactions into different types :(i) $AgNO_3(aq) + NaCl(aq) \rightarrow AgCl(s) + NaNO_3(aq)$(ii) $CaO(s) + H_2O(l) \rightarrow Ca(OH)_2 (aq)$(iii) $2KClO_3(s) \rightarrow 2KCl(aq) + 3O_2 (g)$(iv) $Zn + CuSO_4 \rightarrow ZnSO_4 + Cu$(b) Translate the following statement into a balanced chemical equation : ‘‘Barium chloride reacts with aluminium sulphate to give aluminium chloride and barium sulphate.’’
(a) (i) $AgNO_3(aq) + NaCl(aq) \rightarrow AgCl(s) + NaNO_3(aq)$:- This is a double displacement reaction as the two reactants exchange their ions to form new compounds. The general format is: AB + CD ⇢AD + CB.A
A solid precipitate of silver chloride along with aqueous sodium nitrate, both of which together gives a milky white suspension. As a precipitate is formed, it is also known as precipitation reaction.
(ii) $CaO(s) + H_2O(l) \rightarrow Ca(OH)_2 (aq)$:- This is a Combination Reaction as two reactants combine to produce a product. As Calcium oxide reacts with slaked lime a ‘hissing sound’ is produced because of the heat released and hence it is also an exothermic reaction.
(iii) $2KClO_3(s) \rightarrow 2KCl(aq) + 3O_2 (g)$:- This is a decomposition reaction where potassium chlorate upon heating undergoes thermal decomposition reaction to form the potassium chloride and oxygen.
(iv) $Zn + CuSO_4 \rightarrow ZnSO_4 + Cu$:- This is a displacement reaction where zinc displaces the copper in copper sulphate to form zinc sulphate and copper. As copper gets reduced and zinc gets oxidized, it is also a redox reaction.
(b) Barium chloride solution reacts with aluminium sulphate solution to form a precipitate of barium sulphate and aluminium chloride solution.
The balanced equation is given as:
$3BaCl_{2} \ ( aq) \ +\ Al_{2}( SO_{4})_{3\ }( aq) \ \rightarrow \ 3BaSO_{4} \ ( s) \ +\ 2AlCl_{3} \ ( aq)$
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