Titration curves for 0.1M solutions of three weak acids ${H A}_{1}$ , ${H A}_{2}$ ans ${H A}_{3}$ with ionization constants $K_{1}$ , $K_{2}$ and $K_{3}$ respectively are plotted in the figure.which of the following is/are true?

K_{2} = (K_{1} + K_{3}) / 2

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K_{1} < K_{3}

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K_{1} > K_{2}

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K_{2} > K_{3}

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Solution

The correct option is A $K_{2} = (K_{1} + K_{3}) / 2$
From the given data $H A_{1}, H A_{2}, H A_{3}$ solutions have same concentration $0.1 M$ .
From the graph it is proved that $K_{2} = (\frac{K_{1} + K_{3}}{2})$

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Titration curves for 0.1M solutions of three weak acids HA1,HA2 ans HA3 with ionization constants K1,K2 and K3 respectively are plotted in the figure.which of the following is/are true?

The correct option is A K2=(K1+K3)/2From the given data HA1,HA2,HA3 solutions have same concentration 0.1M .From the graph it is proved that K2=(K1+K32)

Titration curves for 0.1M solutions of three weak acids ${H A}_{1}$ , ${H A}_{2}$ ans ${H A}_{3}$ with ionization constants $K_{1}$ , $K_{2}$ and $K_{3}$ respectively are plotted in the figure.which of the following is/are true?

The correct option is A $K_{2} = (K_{1} + K_{3}) / 2$
From the given data $H A_{1}, H A_{2}, H A_{3}$ solutions have same concentration $0.1 M$ .
From the graph it is proved that $K_{2} = (\frac{K_{1} + K_{3}}{2})$