1. Principle of the experiment

   In the kinetic study of iodide ion with hydrogen peroxide, iodine is produced:

   $\mathrm{H_2O_2 + 2I^- + 2H^+ \rightarrow I_2 + 2H_2O}$

   The liberated iodine reacts with sodium thiosulphate:

   $\mathrm{I_2 + 2S_2O_3^{2-} \rightarrow 2I^- + S_4O_6^{2-}}$

   As long as thiosulphate is present, iodine is consumed and no blue colour appears with starch. Once thiosulphate is exhausted, free iodine accumulates and gives a blue starch-iodine complex.

2. Examine each statement

   (A) Always use freshly prepared starch solution.

   This is correct. Starch solution decomposes on standing and may not give a sharp blue colour reliably.

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   (B) Always keep the concentration of sodium thiosulphate solution less than that of KI solution.

   This is correct in practice for the iodine clock-type kinetic study. KI must be in sufficient excess, while thiosulphate is kept smaller so that only a small fixed amount of iodine is removed before the blue colour appears. This allows a measurable induction time.

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   (C) Record the time immediately after the appearance of blue colour.

   This is taken as correct experimentally. The observed endpoint is the appearance of blue colour, so the time is recorded at that instant (practically, immediately after observing it).

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   (D) Record the time immediately before the appearance of blue colour.

   This is incorrect. One cannot experimentally mark the endpoint before the colour appears; the measurable event is the appearance of blue colour.

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   (E) Always keep the concentration of sodium thiosulphate solution more than that of KI solution.

   This is incorrect. If thiosulphate were too large, iodine formed would continue to be consumed for too long, delaying or disturbing the endpoint. It is not kept more than KI.

3. Correct set of statements

   Correct statements are:

   $\boxed{(A), (B), (C)}$

4. Match with options

   Option A corresponds to:

   $\boxed{(A),(B),(C)\text{ only}}$

Hence, the correct answer is Option A.