Question

What is the pH of a 0.320 M solution of hypobromous acid (HBrO)? Ka = 2.8 ✕ 10-9

Answer 1

hey mate, here is ur answer

Answer

For most weak acid problems, [H3O+] = sqrt (Ka x [HA]o)

[H3O+] = sqrt ((2.8 x 10^-9)(0.216)) = 2.5 x 10^-5 M

pH = -log [H3O+] = -log (2.5 x 10^-5) = 4.61

Answer 2

The pH of the solution is 4.52

Explanation:

We are given:

Molarity of hypobromous acid = 0.320 M

The chemical equation for the ionization of hypobromus acid follows:

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

Initial:               0.320        

At eqllm:         0.320-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:

$2.8\times 10^{-9}=\frac{x\times x}{(0.320-x)}\\\\x=-0.0000299,0.0000299$

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:

$pH=-\log (2.99\times 10^{-5})\\\\pH=4.52$

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