The third dissociation constant of H3PO4 is 1-3 - 10-12- Assume that the hydrolysis proceeds only in the first step- the pH of 0-1 M K3PO4 solution is-

The correct option is B pH=12.44 For a salt of weak acid amp; strong base (K_3PO_4) , pH=7+12(pK_a+log C) =7+12[ log(1.3× 10^ 12)+log0.1] ...

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pH of a Solution

The third dis...

Question

The third dissociation constant of $H_{3} P O_{4}$ is $1.3 \times 10^{- 12}$ . Assume that the hydrolysis proceeds only in the first step, the $p H$ of $0.1 M K_{3} P O_{4}$ solution is:

p H = 13.12

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p H = 12.44

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p H = 12.64

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p H = 12.49

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Solution

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Similar questions

0.1 M K_{3} P O_{4}

25^{\circ} C

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1.3 \times 10^{- 12}

l o g (4.6) = 0.66

p H

0.1 M

K_{3} {P O}_{4}

H_{3} {P O}_{4}

1.3 \times 10^{- 12}

H_{3} P O_{4}

1.5 \times 10^{- 4} ?

p H

H_{2} P O_{4}^{-}

K_{a_{1}}

H_{3} P O_{4}

K_{a_{2}}

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The degree of hydrolysis and pH of $0.1 M$ sodium acetate solution are:
Hydrolysis constant of sodium acetate is $5.6 \times 10^{- 10}$ .

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