For the reaction B- - H2O- BOH - H- kb for BOH is 1- 10-6- If the value of hydrogen constant is 1- 10-x- Then value of x is

Hydrogen Constant ⟶ Hydrolysis Constant =K_wK_b=[ H ^ + ] [ OH ^ ] #160; K _ b = 10 ^ 14 10 ^ 6 = 10 ^ 8 x=8 ...

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pH the Power of H

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For the reaction $B^{+} + H_{2} O ⇌ B O H + H^{+}, k b$ for $B O H$ is $1 \times 10^{- 6}$ . If the value of hydrogen constant is $1 \times 10^{- x}$ . Then value of $x$ is

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K_{b}

B^{+} + H_{2} O ⇌ B O H + H^{+}

1.0 \times 10^{- 6}

K_{b}

B^{+} + H_{2} O ⇌ B O H + H^{+}

1.0 \times 10^{- 6}

B O H ⇌ B^{\oplus} + ⊝ O H

25^{o} C

2.5 \times 10^{- 6}

B O H + H^{\oplus} ⇌ B^{\oplus} + H_{2} O

B^{+} + H_{2} O ⇌ B O H + H^{+}

K_{b} = 1 \times 10^{- 5}

In the hydrolytic equilibrium;

$B^{+} + H_{2} O ⇌ B O H + H^{+}$

$K_{b}$ = $1 \times 10^{- 5}$ . The hydrolysis constant is-

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