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Calculate the ph when 20.0 ml of 0.150 m koh is mixed with 20.0 ml of 0.300 m hbro (ka = 2.5 × 10⁻⁹)

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The pH of the solution is 10.74. the pH refers to the hydrogen ion concentration. It is a measure of the acidity of the solution.

What is pH?

pH is the degree of acidity or alkalinity of a solution.

The equation of the reaction is;

KOH + HBrO ==> KBrO + H2O

The number if moles of KOH =20.0 ml x 1 L / 1000 ml x 0.150 mol/L = 0.003 moles KOH

The number of moles of HBrO = 20.0 ml x 1 L / 1000 ml x 0.300 mol/L = 0.006 moles HBrO

Since the reaction is 1:2;

[BrO-] = 0.003 mols / 0.04L = 0.075M

Now the pH, is obtained from;

KBrO + H2O ==> KOH + HBrO

BrO- + H2O ==> HBrO + OH-  

Kb of BrO- = 1x10-14 / 2.5x10-9 = 4x10-6

Kb = 4x10-6 = [HBrO][OH-] / [BrO-]

From the ICE table;

4x10^-6 = (x)^2 / 0.075

x = 5.48x10-4 M = [OH-]

pOH = -log 5.48x10-4 M = 3.26

pH = 14 - pOH

pH = 10.74

Learn more about pH: https://brainly.com/question/15289741?

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