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At 25^o C, pH of a 0.01M solution of a weak mono basic acid [HA] is 4. The correct statement(s) regarding HA and its given solutions is (are)

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Increasing the temperature of solution would cause the pH to decrease.

Addition of 0.1M HCl solution would lower pH by increasing degree of ionisation.

P^Hof solution becomes 5 when 990ml water is added to 10 ml of same solution.

The ionisation constant (K_a) of acid is approximately 10^–6 at 25^o C

answer is A, B, C.

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Detailed Solution

C = 0.01 M
pH of HA = 4
[H+] = 10^–4
[H+] = $\sqrt{K a \times C}$
$K a = \frac{{[H^{+}]}^{2}}{C} = \frac{10^{- 8}}{10^{- 2}} = 10^{- 6}$

When the temperature increases, [H+] increases, the pH of the solution decreases.

For weak acid

pH after dilution = pH before dilution + $\log_{10} (\sqrt{\frac{V_{f i n a l}}{V_{i n i t i a l}}})$

= 4 + $\log_{10} (\sqrt{\frac{990 + 10}{10}})$

= 4 + 1 = 5

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