The dissociation constant of mono-basic acids A, B and C are $10^{- 4}, 10^{- 6}$ and $10^{- 10}$ respectively. The concentration of each is 0.1 M. Which of the following has been arranged in order of increasing pH ?

A < B < C

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C < B < A

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C < A < B

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B < A < C

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Solution

The correct option is A $A < B < C$
Higher is the value of the dissociation constant $K_{a}$ , stronger is the acid and lower is its pH.

The decreasing order of the acid dissociation constant is $A > B > C$ .

Hence the increasing order of pH is $A < B < C$ .

Option A is correct.

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Similar questions

A, B, C, D

6 \times 10^{- 4}, 5 \times 10^{- 5}, 3.6 \times 10^{- 6}, a n d 7 \times 10^{- 10}

0.1

pH of 0.1 M weak acid solution is 4. What is the dissociation constant of the acid ?

6 \times 10^{4}, 5 \times 10^{5}, 3.6 \times 10^{6} a n d 7 \times 10^{10}

H A

α << 1.

K_{a}

C

B O H

α << 1.

K_{b}

C

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