Consider the following statements (a) The pH of a mixture containing 400 mL of 0.1 M H2SO4 and 400 mL of 0.1 M NaOH will be approximately 1.3. (b) Ionic product of water is temperature dependent. (c) A monobasic acid with Ka = 10–5 has a pH = 5. The degree of dissociation of this acid is 50%. (d) The Le Chatelier's principle is not applicable to common-ion effect. The correct statements are :

Engineering

Chemistry

Le Chateliers Principle

pH Calculation for Acids and Bases

pH Scale and Relative Strength of Acids

Question

Consider the following statements

(a) The pH of a mixture containing 400 mL of 0.1 M H₂SO₄ and 400 mL of 0.1 M NaOH will be approximately 1.3.

(b) Ionic product of water is temperature dependent.

(d) The Le Chatelier's principle is not applicable to common-ion effect.

The correct statements are :

(a), (b) and (c)

(a) and (b)

(b) and (c)

(a), (b) and (d)

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(a) H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O

400×.1=40 400×.1=40

$∴ [H^{+}] = \frac{20 \times 2}{800} = \frac{1}{20} \Rightarrow pH = - \log (\frac{1}{20})$

$∴$ pH = 1.3 so (a) is correct

(b) $log (\frac{{Kw}_{2}}{{Kw}_{1}}) = \frac{ΔH}{2 .303 R} [\frac{1}{T_{1}} - \frac{1}{T_{2}}]$

So ionic product of water is temp. dependent hence (b) is correct.

$K_{a} = \frac{{cα}^{2}}{(1 - α)} \Rightarrow K_{a} = \frac{[H^{+}] . α}{(1 - α)}$

$∴ 10^{- 5} = \frac{10^{- 5} . α}{(1 - α)} \Rightarrow 1 - α = α \Rightarrow α = \frac{1}{2} = 50 %$

so (c) is correct.

(d) Le-chatelier’s principle is applicable to common-ion effect so option (d) is wrong