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What is the pH of the solution that results from the combination of 50.00mL of 0.0200M...

What is the pH of the solution that results from the combination of 50.00mL of 0.0200M HOCl and 25.00mL of 0.0200M KOH? Ka= 3.162x10^-8 for HOCl

Solutions

Expert Solution

millimoles of HOCl = 50 x 0.02 = 1

millimoles of KOH = 25 x 0.02 = 0.5

Ka = 3.162 x 10^-8

pKa = -log Ka

pKa = 7.50

HOCl + KOH -------------------------> KOCl + H2O

1            0.5                                        0           0

0.5         0.0                                     0.5         0.5

millimoles of HOCl = millimoles of KOCl . so it is half equivalence point.

here pH = pKa

pH = 7.50


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