(i) What happens when zinc granules are treated with dilute solution of $H_{2} S O_{4}$ ? Also write the chemical equations if reaction occurs.

(ii) What happens when zinc granules are treated with dilute solution of HCl? Also write the chemical equations if reaction occurs.

(iii) What happens when zinc granules are treated with dilute solution of $H N O_{3}$ ? Also write the chemical equations if reaction occurs.

(iv) What happens when zinc granules are treated with dilute solution of NaCl? Also write the chemical equations if reaction occurs.

(v) What happens when zinc granules are treated with dilute solution of NaOH? Also write the chemical equations if reaction occurs.

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Solution

(i) Zinc granules react with dilute $H_{2} S O_{4}$ to form zinc sulphate and release hydrogen gas.
$Z n (s) + H_{2} S O_{4} (a q) ⟶ Z n S O_{4} (a q) + H_{2} (g)$
This is an example of a single displacement reaction. Zinc being more reactive, displaces hydrogen from the dilute acid.

(ii) Zinc granules react with dilute HCl to form zinc chloride and hydrogen gas.
$2 Z n (s) + 2 H C l (a q) ⟶ Z n C l_{2} (a q) + H_{2} (g)$
This is an example of a single displacement reaction. Zinc being more reactive, displaces hydrogen from the dilute acid.

(iii) Zinc granules react with dilute Nitric acid to form zinc nitrate and nitrous oxide (N2O) gas.
$4 Z n (s) + 10 H N O_{3} (a q) ⟶ 4 Z n (N O_{3})_{2} (a q) + 5 H_{2} O (l) + N_{2} O (g)$
Hydrogen is not obtained as it is oxidized to water by the strongly oxidizing nitric acid.
Metals generally produce hydrogen gas with dilute acids, except for $H N O_{3}$ .

(iv) Sodium is a more reactive metal than zinc, therefore zinc is unable to displace sodium from its salt solution.
$Z n (s) + N a C l (s) ⟶ No reaction$

(v) Zinc granules react with dilute NaOH to form sodium zincate and hydrogen gas.
Zinc is an amphoteric metal, which means it can react with both acids and bases to produce a salt and hydrogen gas.
$Z n (s) + 2 N a O H (a q) ⟶ N a_{2} Z n O_{2} (a q) + H_{2} (g)$

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