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Considering a...

Question

Considering a $0.1 M H_{3} P O_{4}$ solution, answer the questions given below:
[Given : $K_{1} = 7.5 \times 10^{- 3}, K_{2} = 6.2 \times 10^{- 8}, K_{3} = 3.6 \times 10^{- 13}$ ]
In the given solution $[H^{+}]$ & $[H_{2} P O_{4}^{-}]$ is:

A

[H^{+}] = [H_{2} P O_{4}^{-}] = 0.024 M

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B

[H^{+}] = 0.076 M; [H_{2} P O_{4}^{-}] = 0.024 M

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C

[H^{+}] = 0.024 M; [H_{2} P O_{4}^{-}] = 0.012 M

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D

[H^{+}] = [H_{2} P O_{4}^{-}] = 0.076 M

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Solution

The correct option is A $[H^{+}] = [H_{2} P O_{4}^{-}] = 0.024 M$
According to ostwald dilution law-
$H^{=} = \sqrt{K_{a} \times C}$
$H^{+} = \sqrt{7.5 \times 10^{- 3} \times .1} = .024 M$

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Similar questions

H_{3} P O_{4}, H_{3} P O_{4} ⇋ H_{2} P O_{4}^{-} + H^{+} (K_{1})

H_{2} P O_{4}^{-} ⇋ H P O_{4}^{2 -} + H^{+} (K_{2})

H P O_{4}^{2 -} ⇋ P O_{4}^{3 -} + H^{+} (K_{3})

Q. The equilibrium constants for the reactions are

H_{3} P O_{4}_{1} H^{+} + H_{2} P O_{4}^{-}; K_{1}

H_{2} P O_{4}^{-}_{2} H^{+} + H P O_{4}^{2 -}; K_{2}

H P O_{4}^{2 -}_{3} H^{+} + P O_{4}^{3 -}; K_{3}

The equilibrium constant for,

H_{3} P O_{4} ⇌ 3 H^{+} + P O_{4}^{3 -}

Q. Calculate the pH of

0.1

M solution of (i)

N a H C O_{3}

N a_{2} H P O_{4}

N a H_{2} P O_{4}

C O_{2} + H_{2} O ⇌ H^{+} + C O_{3}^{2 -}

K_{1} = 4.2 \times 10^{- 7}

M

H C O_{3}^{-} ⇌ H^{+} + C O_{3}^{2 -}

K_{2} = 4.8 \times 10^{- 11}

M

H_{2} P O_{4} ⇌ H^{+} + H_{2} P O_{4}^{-}

K_{1} = 7.5 \times 10^{- 3}

M

H_{2} P O_{4}^{-} ⇌ H^{+} + H P O_{4}^{2 -}

K_{2} = 6.2 \times 10^{- 8}

M

H P O_{4}^{2 -} ⇌ H^{+} + P O_{4}^{3 -}

K_{3} = 1.0 \times 10^{- 12}

Q. Calculate the

O H^{-}

concentration and the

H_{2} P O_{4}

concentration of a solution prepared by dissolving

0.1

N a_{3} P O_{4}

in sufficient water to make

1

K_{1} = 7.1 \times 10^{- 3}, K_{2} = 6.3 \times 10^{- 8}, K_{3} = 4.5 \times 10^{- 13}

Q. Calculate the equilibrium constants for the reactions with water of

H_{2} P O_{4}^{⊝}, H P O_{4}^{2 -}

P O_{4}^{3 -}

as base. Comparing the relative values of two equilibrium constants of

H_{2} P O_{4}^{⊝}

with water, deduce whether solutions of this ion in water are acidic or bases. Deduce whether solutions of

H P O_{4}^{2 -}

are acidic or bases. Given

K_{1}, K_{2}

K_{3}

H_{3} P O_{4}

7.1 \times 10^{- 3}, 6.3 \times 10^{- 8}

4.5 \times 10^{- 13}

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Standard XII Mathematics