The ionization constant of chloroacetic acid is 1-35- 10 -3- What will be the pH of 0-1 M acid and its 0-1 M sodium salt solution-

(i) For acid solution, [H^+] = √(K_aC) = √(0.00135 × 0.1) = 0.0116M pH = log [H^+] = log 0.0116=1.936 (ii) For 0.1 M sodium salt solution,The solutio ...

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Standard XII

Chemistry

Sulphuric Acid

The ionizatio...

Question

The ionization constant of chloroacetic acid is $1.35 \times 10^{- 3}$ . What will be the $p H$ of 0.1 M acid and its 0.1 M sodium salt solution?

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Solution

(i) For acid solution,
$[H^{+}] = \sqrt{K_{a} C} = \sqrt{0.00135 \times 0.1} = 0.0116 M$
$p H = - l o g [H^{+}] = - l o g 0.0116 = 1.936$
(ii) For 0.1 M sodium salt solution,
The solution contains sodium salt of chloroacetic acid which is weak acid and strong base.
$p K_{a} = - l o g K_{a} = l o g (0.00135) = 2.8697$
$p K_{w} = 14$
$l o g c = l o g 0.1 = - 1$
$p H = 0.5 [p K_{w} + p K_{a} + l o g c] = 0.5 [14 + 2.8697 - 1] = 7.935$

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The ionization constant of chloroacetic acid is 1.35×10−3. What will be the pH of 0.1 M acid and its 0.1 M sodium salt solution?

The ionization constant of chloroacetic acid is $1.35 \times 10^{- 3}$ . What will be the $p H$ of 0.1 M acid and its 0.1 M sodium salt solution?