Calculate the hydrolysis constant $(K_{h})$ of the salt containing $N O_{2}$ . Given the

$K_{a}$ for $H N O_{2}$ = $4.5 \times 10^{- 10}$

$2.22 \times 10^{- 5}$

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$2.02 \times 10^{5}$

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$4.33 \times 10^{4}$

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$3.03 \times 10^{- 5}$

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Solution

The correct option is A
$2.22 \times 10^{- 5}$

$K_{h}$ = $\frac{K_{w}}{K_{a}}$ = $\frac{1 \times 10^{- 14}}{4.5 \times 10^{- 10}}$ = $2.22 \times 10^{- 5}$

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Similar questions

N O_{2}^{-}

K_{a}

H N O_{2} = 4.5 \times 10^{- 10}

Calculate the hydrolysis constant $(K_{h})$ of the salt containing $N O_{2}$ . Given the

$K_{a}$ for $H N O_{2}$ = $4.5 \times 10^{- 10}$

N O_{2}^{-}

K_{a}

H N O_{2} = 4.5 \times 10^{- 10}

(K_{h})

K_{a} =

1.8 \times

10^{- 5}

K_{b} =

2 \times

10^{- 5}

K_{w} = 10^{- 14}

(K_{h})

25^{\circ} C ?

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