a 100ml sample of .20M HF is titrated with .10M KOH. determine Ph of solution after...

a 100ml sample of .20M HF is titrated with .10M KOH. determine Ph of solution after addition of 100ml of KOH.Ka is 3.5x10-4.

Expert Solution

millimoles of HF = 100 x 0.20 = 20

millimoles of KOH = 100 x 0.10 = 10

HF + KOH --------------------> KF + H2O

20 10 0 0 ----------------------> initial

10 0 10 0 -----------------------> after reaction

in this mixture HF weak acid and KF salt remained . so it can form acidic buffer

pKa = -log Ka = -log(3.5x10^-4.) =3.46

For acidic buffer

Henderson-Hasselbalch equation

pH = pKa + log[salt/acid]

pH = 3.46 + log (10/10)

pH = 3.46

queen_honey_blossom answered 2 years ago

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