(a)
(i) Acids are compounds that generate hydronium ions (the only positively charged ions) when they get dissolved in water. Examples include hydrochloric acid (HCl) and sulphuric acid ().
HCl + H2O ⇌ H3O+ + Cl-
(ii) pH scale is defined as the scale of acidity that is used to determine the acidic or basic (alkaline) nature of a solution. On the pH scale, bases (or alkalis) have a pH value greater than 7, while acids have a pH value less than 7. Neutral solutions have the pH value 7.
(iii) The reaction between an acid and a base to form a salt and water is called neutralisation reaction. For example, hydrochloric acid reacts with sodium hydroxide to form sodium chloride and water.
NaOH + HCl →NaCl + H2O
Normal salt
(b) (i) and (ii) Preparation of lead chloride from lead oxide involves the following steps:
Step I: Lead (II) oxide (insoluble) is treated with dilute nitric acid to form soluble lead nitrate.
PbO + 2HNO3 → Pb(NO3)2 + H2O
Insoluble Soluble
Step II: Lead nitrate is then treated with hydrochloric acid to form insoluble lead (II) chloride and water.
Pb(NO3)2 + 2HCl →PbCl2 + 2HNO3
Insoluble
(iii) When iron metal reacts with dilute sulphuric acid, it forms iron (II) sulphate or ferrous sulphate and releases hydrogen gas.
(iv) On the pH scale, bases (or alkalis) have a pH value greater than 7, while acids have a pH value less than 7. Therefore, iron (III) chloride solution with a pH value less than 7 is acidic in nature.