A tribasic acid, $H_{3} A$ , dissociates into a dibasic acid, $H_{2} B$ and a monobasic acid, HC, obeying first order kinetics.
$H_{3} A ⟶ H_{2} B + HC; k = 0.04 \min^{- 1}$
The kinetics is studied by withdrawing a definite volume (5 ml) of the reaction mixture at different times and titrating it with 0.4 M $NaOH$ solution. If the volume of $NaOH$ solution needed for complete titration at t = 0 is 25 ml, then the volume (in ml) of $NaOH$ solution needed for titration at t = 25 min is:

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answer is 25.

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Detailed Solution

In the reaction we have,

$H_{3} A ⟶ H_{2} B + HC$

$\begin{array}{cccc} t = 0 & a & - x \\ t = i & a - x & x & x \end{array}$

$0.4 \times 25 \propto 3 a$

At time t,

$\begin{array}{l} (α - x) \times 3 + x \times 2 + x \times 1 \\ 3 a \propto 0.4 \times 25 \end{array}$

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