(a) (i) Define a base according to Arrhenius concept.

(ii) Give one example of an Arrhenius base.

(iii) Identify each of the following substances in aqueous solutions as strong electrolyte, non-electrolyte or weak electrolyte.

I. C\(_{12}\)H\(_{22}\)O\(_{11}\)  II. NH\(_3\) Ill. NaOH

(iv) Write a balanced equation to represent the reaction between CH\(_3\)COOH and KOH.

(b) Calculate the volume of 0.500 mol dm\(^{-3}\) HCI required to neutralize 20.00 cm\(^3\) of 0.300 mol dm\(^{-3}\) NaOH.

(c) Give the IUPAC name of each of the following salts: (ii) NaOCI; (iii) Mg(HCO\(_3\))\(_2\).

(d)(i) Define the term standard solution.

(ii) Consider the following compounds: NaOH and Na\(_2\)CO\(_3\). Which of the compounds is suitable for the preparation of a standard alkaline solution? Give reason for your answer

(iii) Fe completely reacted with dilute HCI.

I. Write an equation for the reaction

II. If 3.08g of Fe completely reacted with 50.0 cm\(^3\) of 2.20 mol dm\(^{-3}\) HCI, calculate the relative atomic mass of the metal.

(a)(i) Give the two reasons why soda lime is used instead of caustic soda in the preparation of methane.

(ii) List two physical properties of methane.

(iii) A hydrocarbon with a vapour density of 29 contains 82.76% carbon and 17.24% hydrogen. Determine the: I. empirical formula; II. molecular formula of the hydrocarbon. [ H = 1.00 C = 12.00 ]

(b)(i) What is meant by the term isomerism?

(ii) Draw the structures of the two isomers of the compound with the molecular formula C\(_2\)H\(_6\)O.

(iii) Give the name of each of the isomers in (b)(ii).

(iv) State the major difference between the isomers.

(c) Give three deductions that could be made from the qualitative and quantitative analysis of a given organic compound.

(d) Give one chemical test to distinguish between propene and propane.

(a (i) Explain why water is referred to as a universal solvent.

(ii) Give one chemical test for water. H\(_2\)SO\(_4\)

(b) A current of 1.25A was passed through an electrolytic cell containing dil.  for 40 minutes.

(i) Write (ii) Calculate the volume of gas produced at the anode at s.t.p. (1F = 96,500 C, Molar Volume of gas at s.t.p. = 22.4 dm\(^3\) mol\(^{-3}\) ]

(C) Consider the reaction represented by the following equation: Au\(_{(s)}\) + Cl\(_{2(g)}\) \(\to\)  AuCl\(_{3(s)}\)

(I) Balance the equation

(ii) If 1.2509 of Au and 1.744g of Cl\(_2\) were mixed

I. determine which of the reactants is in excess II. calculate the excess amount [Au = 197.0, CI = 35.5]

(a) Name one product of destructive distillation of coal that is (i) solid (ii) liquid; (iii) gas.

(b) (i) What is the major component of synthetic gas? (ii) Give one reason why synthetic gas is not a major source of air pollution.

(c) (i) Write a balanced chemical equation for the complete combustion of carbon. (ii) State two: I. physical; II. chemical properties of the product in (c)(i).

(d) (i) Name two allotropes of carbon that are I. crystalline, II. amorphous. (ii) State one use of each of the allotropes named in (d)(i).

(e) (i) By means of balanced chemical equations only, outline the process of manufacture of H\(_2\)SO\(_4\), by contact process.

(ii) State the function of H\(_2\)SO\(_4\) in each of the following reaction equations:

I.  C\(_2\)H\(_5\)OH\(_{2(l)}\)  \(\to\) C\(_2\)H\(_{4(g)}\);

II. Pb(NO\(_{3(g)}\) + H\(_2\)SO\(_{4(g)}\) —> PbSO\(_{4(s)}\) + 2HNO\(_{3(aq)}\)

(a) An aqueous solution of salt Q was added to excess Sodium trioxocarbonate (V) solution in a test tube. There was effervescence, the test tube became warm and a white precipitate was observed. State three inferences that could be drawn from these observations.

(b) Consider the following salts: NH\(_4\)CI; PbSO\(_4\); NaHCO\(_3\), Cu(NO\(_3\))\(_2\) and ZnCO\(_3\). Select from the list, the salt(s) which;

(i) do not/does not readily dissolve in water;

(i) produce(s) effervescence with dilute mineral acids;

(ii) decompose(s) on heating

(iv) dissolves(s) in water to form an alkaline solution;

(v) sublime(s) on heating.