The dissociation constants of two acids- HA1 and HA2- are 4-5 - 10-4 and 1-8 - 10-5 respectively- If both are having equal concentrations- then the relative strength of the acids is-

The correct option is B 5:1 The dissociation of acid is given by the following equation: #160; HA → H^+ + A^ The given acids have a very low dissoc ...

The dissociat...

Question

The dissociation constants of two acids, $H A_{1}$ and $H A_{2}$ , are $4.5 \times 10^{- 4}$ and $1.8 \times 10^{- 5}$ respectively. If both are having equal concentrations, then the relative strength of the acids is:

5 : 2

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2 : 5

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5 : 1

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1 : 5

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Solution

The correct option is B $5 : 1$
The dissociation of acid is given by the following equation: $H A \to H^{+} + A^{-}$

The given acids have a very low dissociation constant, i.e., the $H A$ concentration can be assumed to be unchanged.

Therefore, $[H^{+}] = \sqrt{\frac{K_{a}}{c}}$ .
Since, the concentration is assumed to be constant, the relative strength $= \frac{H_{H A_{1}}^{+}}{H_{H A_{2}}^{+}} = \sqrt{\frac{45}{1.8}} = 5 : 1$ .

Option C is correct.

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