Calculate the pH of a solution that is 060M HF and 100M KF a

Calculate the pH of a solution that is 0.60-M HF and 1.00-M KF

(according to the question in the book, there was no Ka value given)

Solution

Ka of HF = 6.3×10^–4

pKa = -log Ka = 3.20

concentration of HF = 0.60 M

concentration of KF = 1.00 M

pH = pKa + log [salt / acid]

     = 3.20 + log [1.00 / 0.60]

pH = 3.42