(a) A soluble chloride X reacted with a liquid Y on heating, to give gas Z which turned moist blue litmus paper red and fumed in moist air.

(i) Identity Y and Z 

(ii) Give one chemical test to confirm that X is a chloride

(b)(i) State one laboratory use of calcium chloride.

(ii) Name one laboratory technique suitable for separating a mixture of iron filings and ammonium chloride without applying heat.

(iii) State the action of solutions of the following salts on litmus respectively: K\(_2\)CO\(_3\);  NaNO\(_3\), AICl\(_3\), (NH\(_4\))\(_2\)SO\(_4\).

Credit will be given for strict adherence to instructions, for observations precisely recorded, and for accurate inferences. All tests, observations, and inferences must be clearly entered in your answer book, In ink, a the time they are made.

C is a mixture of two simple salts. Carry out the following exercises on C. Record your observations and identify any gases evolved. State the conclusion you draw from the result of each test.

(a) Add about 10cm\(^3\) of distilled water to all of C in a boiling tube. Shake the mixture and filter: Keep both the filtrate and the residue.

(b) Divide the filtrate into two portions.

(i) To the first portion, add about 2cm\(^3\) of barium chloride solution, followed by dilute hydrochloric acid in excess. Warm the mixture and identify any gas evolved.

(ii) To the second portion, add few drops of acidified potassium tetraoxomanganate (VIl) solution and shake.

(C) Put the residue in a test tube and add about 3cm\(^3\) of dilute hydrochloric acid Warm gently and identify any gas evolved. Keep the mixture.

(d) Divide the clear solution from (c) above into two portions

(i) To the first portion, add sodium hydroxide solution in drops and then in excess.

(ii) To the second, add aqueous ammonia in drops and then in excess.

All your burette readings (initial and final), as well as the size of your pipette, must be recorded but no account of experimental procedure is required. All calculations must be done in your answer book.

A is a solution containing 14.0gdm\(^{-3}\) of potassium hydrogen tetraoxosulphate (VI). B is a solution of sodium hydroxide.

(a) Put A into the burette and titrate with 20.0cm\(^{-3}\) or 25.0 cm\(^{-3}\) portion of B using methyl orange, as Indicator. Record the volume of your pipette. Tabulate your burette readings and calculate the average volume of A used.

(b) From your results and the information provided, calculate the:

(i) concentration of A in mol dm\(^{3}\)

(ii) concentration of B in g dm\(^3\)

(iii) volume of A (in dm\(^{-3}\)) that would produce one mole of Sodium tetraoxosulphate (VI) in solution. The equation for the reaction is:

2KHSO\(_{4(aq)}\) + 2NaOH\(_{(aq}\) \(\to\) K\(_2\)SO\(_{4(aq)}\) + NaSO\(_{4(aq)}\) + 2H\(_2\)O\(_{(l)}\) [H = 1; O = 16, Na = 23, KHSO\(_4\) =  136gmol\(^{-2}\)]