(a) (i) to some dil. HCI in a beaker, add Zn granules and shake.
(ii) continue to add Zn granules un effervescence stops and the Zn is in excess.
(iii) filter off undissolved Zn granules
(iv) put the filtra in an evaporating dish and heat to concentrate.
(v) cool to obtain crystals (vi) filter and dry the crysta between filter papers.
(ii) Zn\(_{(s)}\) + 2HCI\(_{(aq)}\) \(to\) ZnCl\(_{2(aq)}\) + H\(_{2(g)}\)

(b)(i) CH\(_3\)COOK\(_{(aq)}\)
(ii) Na\(_2\)SO\(_{4(aq)}\)
(iii) Pb(NO\(_3\))\(_{2(aq)}\) and MgCl\(_{2(aq)}\)

(c)(i) I. MnO\(_2\)
Mn + (-2 x 2) = O
Mn — 4 = 0
Mn = + 4
(ii) KMnO\(_4\)
1 + Mn + (– 2 x 4) = 0
1 + Mn – 8 = 0
Mn = + 7

(ii) MnO\(_2\) – as a catalyst
– as an oxidizing agent
KMnO\(_4\) – as an oxidizing agent

(d) Oxidation is a process of electron loss, while reduction is a process of electron gain. A species can only be oxidized if there is another species that would readily accept the donated electron(s)/ Hence every oxidation must be accompanied by a reduction.

(e) (i) I. Fe\(_{(s)}\) \(\to\) F\(^{2+}_{(aq)}\) + 2e\(^-\)
II. Ag\(^+_{(aq)}\) + e\(^-\) \(\to\) Ag\(_{(s)}\)
(ii) I. Fe is oxidized II. Ag\(^+\) is reduced
(iii) +1 to 0.