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

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

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

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

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K_{1} . K_{2} . K_{3} = K_{w}

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Solution

The correct option is B $K_{1} > K_{2} > K_{3}$
$H_{3} P O_{4} ⇋ H_{2} P O_{4}^{-} + H^{+}$

$K_{1} = \frac{[H_{2} P O_{4}^{-}] [H^{+}]}{[H_{3} P O_{4}]}$
$K_{2} = \frac{[H P O_{4}^{2 -}] [H^{+}]}{[H_{2} P O_{4}^{-}]}$

$K_{3} = \frac{[P O_{4}^{3 -}] [H^{+}]}{[H P O_{4}^{2 -}]}$

$K_{1} > K_{2} > K_{3}$ as it depends on more $H^{+}$ ions

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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 :

For $C u^{2 +}$ ion in $[C u (H_{2} O)_{4} (e n)]^{2 +}, [C u (H_{2} O)_{2} (e n)_{2}]^{2 +}$ and $[C u (e n)_{3}]^{2 +}$ with the stability constant $k_{1}, k_{2}$ and $k_{3}$ respectively, which of the following holds true?

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:

If $k_{1}, k_{2}, k_{3}$ are real numbers and the equation $k_{1} x^{2} + k_{2} x + k_{3} = 0$ have three roots, then value of $k_{1} + k_{2} + k_{3}$ is

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For H3PO4,H3PO4⇋H2PO−4+H+(K1)H2PO−4⇋HPO2−4+H+(K2)HPO2−4⇋PO3−4+H+(K3), then

The correct option is B K1>K2>K3H3PO4⇋H2PO−4+H+K1=[H2PO−4][H+][H3PO4]K2=[HPO2−4][H+][H2PO−4]K3=[PO3−4][H+][HPO2−4]K1>K2>K3 as it depends on more H+ ions

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