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Standard XII

Chemistry

Concentration Terms

What would be...

Question

What would be the pH of an ammonia solution if that of an acetic acid solution of equal strength is 3.2? Assume dissociation constant for $N H_{3}$ $&$ acetic acid are equal.

3.2

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6.4

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9.6

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10.8

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Solution

The correct option is D 10.8
If $K_{a}$ for acetic acid $= k_{b}$ for $N H_{3}$ then for solution of equal strength
${[H_{3} O^{+}]}_{A C O H}^{+} = {[O H^{-}]}_{N H_{3}}^{-}$
pH of ACOH solution = pOH of $N H_{3}$ solution
pH of $N H_{3}$ solution = 14 – 3.2 = 10.8

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What would be the pH of an ammonia solution if that of an acetic acid solution of equal strength is 3.2? Assume dissociation constant for NH3 & acetic acid are equal.

The correct option is D 10.8If Ka for acetic acid =kb for NH3 then for solution of equal strength [H3O+]ACOH=[OH−]NH3 pH of ACOH solution = pOH of NH3 solution pH of NH3 solution = 14 – 3.2 = 10.8

What would be the pH of an ammonia solution if that of an acetic acid solution of equal strength is 3.2? Assume dissociation constant for $N H_{3}$ $&$ acetic acid are equal.

The correct option is D 10.8
If $K_{a}$ for acetic acid $= k_{b}$ for $N H_{3}$ then for solution of equal strength
${[H_{3} O^{+}]}_{A C O H}^{+} = {[O H^{-}]}_{N H_{3}}^{-}$
pH of ACOH solution = pOH of $N H_{3}$ solution
pH of $N H_{3}$ solution = 14 – 3.2 = 10.8