Question

What is the pH of a 0.309 M solution of hypobromous acid (HBrO)? Ka = 2.8 ✕ 10-9

Answer 1

sorry brother don't know

Answer 2

The pH of the solution is 4.53

Explanation:

We are given:

Molarity of hypobromous acid = 0.309 M

The chemical equation for the ionization of hypobromus acid follows:

                        $HBrO\rightleftharpoons H^++BrO^-$

Initial:                0.309      

At eqllm:         0.309-x     x        x

The expression of equilibrium constant for above equation follows:

$K_a=\frac{[H^+][BrO^-]}{[HBrO]}$

We are given:

$K_a=2.8\times 10^{-9}$

Putting values in above expression, we get:

$2.8\times 10^{-9}=\frac{x\times x}{(0.309-x)}\\\\x=-0.0000294,0.0000294$

Neglecting the negative value of 'x' because concentration cannot be negative

To calculate the pH of the solution, we use the equation:

$pH=-\log [H^+]$

Putting values in above equation, we get:

$pH=-\log (2.94\times 10^{-5})\\\\pH=4.53$

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