Consider the equilibrium reactions- H3PO4-K1H-H2PO-4 H2PO4-K1H-HPO-24 H-2PO4-K1H-HPO-34The equilbrium constant- K for the following dissociation H3PO4-3 H-PO4-3 is

The correct option is B K_1K_2K_3 K_1=[H^+][H_2PO_4^ ][H_3PO_4],K_2=[H^+][HPO_4^2 ][H_3PO_4^ ], K_3=[H^+][PO_4^3 ][H_2PO_4^ ] ⇒ K_1× K_2× K_3=[H^ ...

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Byju's Answer

Standard XII

Chemistry

Molality

Consider the ...

Question

Consider the equilibrium reactions,
$H_{3} P O_{4} ⇌ K_{1} H^{+} + H_{2} P O_{4}^{-}$
$H_{2} P O_{4} ⇌ K_{1} H^{+} + H P O_{4}^{- 2}$
$H_{- 2} P O_{4} ⇌ K_{1} H^{+} + H P O_{4}^{- 3}$
The equilbrium constant, $K$ for the following dissociation
$H_{3} P O_{4} ⇌ 3 H^{+} + P O_{4}^{- 3}$ is

K_{1} / K_{2} K_{3}

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K_{1} K_{2} K_{3}

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K_{2} / K_{1} K_{3}

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K_{1} + K_{2} + K_{3}

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Solution

The correct option is B $K_{1} K_{2} K_{3}$
$K_{1} = \frac{[H^{+}] [H_{2} P O_{4}^{-}]}{[H_{3} P O_{4}]}, K_{2} = \frac{[H^{+}] [H P O_{4}^{2 -}]}{[H_{3} P O_{4}^{-}]}, K_{3} = \frac{[H^{+}] [P O_{4}^{3 -}]}{[H_{2} P O_{4}^{-}]}$
$\Rightarrow K_{1} \times K_{2} \times K_{3} = \frac{[H^{+}]^{3} [P O_{4}^{3 -}]}{H_{3} P O_{4}}$ .

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Similar questions

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 -}

will be :

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, $H_{3} P O_{4} ⇌ 3 H^{+} + P O_{4}^{3 -}$ will be:

Q. For

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})

, then

Q. The following equilibrium are given

N_{2} + 3 H_{2} \to 2 N H_{3} - K_{1}

N_{2} + O_{2} \to 2 N O - K_{2}

H_{2} + 1 / 2 O_{2} \to H_{2} O - K_{3}

The equilibrium constant of reaction,

3 H_{2} + 5 / 2 O_{2} \to 2 N O + 3 H_{2} O

, in terms of

K_{1}, K_{2}, K_{3}

Q. What is the relation between the equilibrium constants

K

K_{1}

and

K_{2}

for the following reactions?

N_{2} + 2 O_{2} ⇋ 2 N O_{2}, K

N_{2} + O_{2} ⇋ 2 N O, K_{1}

2 N O + O_{2} ⇋ 2 N O_{2}, K_{2}

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Consider the equilibrium reactions,H3PO4⇌K1H++H2PO−4H2PO4⇌K1H++HPO−24H−2PO4⇌K1H++HPO−34The equilbrium constant, K for the following dissociation H3PO4⇌3 H++PO−34 is

The correct option is B K1K2K3K1=[H+][H2PO−4][H3PO4],K2=[H+][HPO2−4][H3PO−4],K3=[H+][PO3−4][H2PO−4]⇒K1×K2×K3=[H+]3[PO3−4]H3PO4 .

Consider the equilibrium reactions,
$H_{3} P O_{4} ⇌ K_{1} H^{+} + H_{2} P O_{4}^{-}$
$H_{2} P O_{4} ⇌ K_{1} H^{+} + H P O_{4}^{- 2}$
$H_{- 2} P O_{4} ⇌ K_{1} H^{+} + H P O_{4}^{- 3}$
The equilbrium constant, $K$ for the following dissociation
$H_{3} P O_{4} ⇌ 3 H^{+} + P O_{4}^{- 3}$ is