For a 21.2 mL sample of a 0.411 M aqueous hydrofluoric acid solution, the pH after 17.6 mL of barium hydroxide has been added is mathematically given as
pH=3.332
What is the pH after 17.6 mL of barium hydroxide has been added?
Generally, the equation for the mole of HF is mathematically given as
mole of HF=molarity*volume
Therefore
mole of HF=0.361*19.2
mole of HF=6.931mmol
The chemical equation
HF+kOH⇆KF+H2O
Therefore
pH=pKa+log(Kf/HF)
pH=3.15+log(6.931*53.6/53.6*4.558)
pH=3.332
In conclusion, The pH
pH=3.332
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