When a 27.7 mL sample of a 0.400 M aqueous hypochlorous acid solution is titrated with a 0.335 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration

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14-03-2022
Chemistry

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When a 27.7 mL sample of a 0.400 M aqueous hypochlorous acid solution is titrated with a 0.335 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration

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okpalawalter8 okpalawalter8 · Answer 1 · 2022-03-28T11:21:56+02:00

With a 27.7 mL sample of a 0.400 M aqueous hypochlorous acid solution titrated with a 0.335 M aqueous potassium hydroxide solution, the pH value is mathematically given as

pH=12.90

What is the pH at the midpoint in the titration?

Moles of HClO=0.329*21.5

Moles of HClO=7.0735

and

Moles of KOH=0.456*23.3

Moles of KOH=10.6248

Hence

The net mole of KOH=10.6248-7.0735

The net mole of KOH=3.5513

Volume of solution=21.5+23.3

Volume of solution=44.8ml

Generally, the equation for the Concentration of KOH is mathematically given as

CKOH=mole/volume

Therefore

CKOH=3.5513/44.8ml

CKOH=0.07927M

In conclusion,

pOH=-log{OH-}

pOH=-log{0.07927}

pOH=1.10

pH=14-110

pH=12.90