chemistry
posted by jaycab on .
COMMON ION EFFECT
1.) What is the pH of a solution that is 0.30M in HCOOH and 0.52M in HCOOK.
Ka of HCOOH=1.7x10^4.
2.) Calculate the pH of a buffer system containing 1.0M CH3COOH and 1.0M CH3COONa. Ka of CH3COOH=1.8x10^5.

1)
I notice that your value for Ka in the question is missing units, were these missing in the original question?
Start from the equation for the equilibrium reaction
HCOOH<>H+ + HCOO
at start
0.30M
at equilibrium if [H+]=x
0.30x x x
there is also 0.52M HCOO
so at equilibrium
0.30x x x+0.52
Ka=[H+][HCOO]/[HCOOH]
Ka=(x)(x+0.52)/(0.30x)=1.7x10^4
(x)(x+0.52)/(0.30x)=1.7x10^4
You can either solve the quadratic or we can say that if x is small with respect 0.52 abd 0.3, we can rewrite the expression as
(x)(0.52)/(0.30)=1.7x10^4
and find x
pH is then log (x/mol litre^1)