Question

The ph of a 0. 50 m solution of base b is found to be 10. 19. what is the kb of the base? the equation described by the kb value is b(aq) h2o(l)↽−−⇀bh (aq) oh−(aq)

Answer 1

The pH of a 0.50 M solution of base B is found to be 10.19. The Kb of the base is 4.8 × 10⁻⁸.

Let's consider the following basic reaction.

B(aq) + H2O(l) ⇄ BH(aq) + OH⁻(aq)

First, we will calculate the pOH of the solution using the following expression. (14-10.19)=3.81

antilog -3.81=1.55×10^-4/0.50=4.8×10^-8

The pH of a 0.50 M solution of base B is found to be 10.19. The Kb of the base is 4.8 × 10⁻⁸.

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Answer 2

The $K_b$ of the base b is 4.805 × 10⁻⁸.

What is dissociation constant?

The dissociation constant is a type of equilibrium constant that measures the degree of dissociation of a salt.

$K_a$ is the dissociation constant for the acid which describes the strength of an acid.

$K_b$ is the dissociation constant of the base which describes the strength of a base.

pOH = 14 - pH = 14 - 10.19 = 3.81

pOH = -log[OH⁻]

3.81 = -log[OH⁻]

Antilog (-3.81) = [OH⁻]

[OH⁻] = 1.55 × 10⁻⁴

Here,

$K_b= \frac{[BH^+][OH^-]}{[B]}$

     = $\frac{(1.55\times10^{-4})(1.55\times10^{-4})}{0.50}$

     = 4.805 × 10⁻⁸

The Kb of the base b is 4.805 × 10⁻⁸

Learn more about dissociation constant:

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