Question

What is the ph of 1m ch3coona solution (ch3cooh ka=1.8×10-5)?

Answer 1

Answer:

[H+]= $\sqrt{ka * c}$

     =$\sqrt{1.8*10^{-5} *1}$

     ≈$4.4*10^{-3}$

pH= -log([H+])

     = -log($4.4*10^{-3}$)

     = 3- 0.643

     = 2.35