Question
In: Chemistry
Calculate the ph of 0.125M of NaAc
Calculate the ph of 0.125M of NaAc
Solutions
Expert Solution
The give compound is a salt of sodium acetate (CH3COO-Na+)
The Ka of acetic acid = 1.8 X 10^-5
So Kb of acetic acid = Kw / Ka = 10^-14 / 1.8X 10^-5 = 5.56 X 10^-10
It will dissociate as
CH3COONa => CH3COO- + Na+
Now
CH3COO- + H2O <------> CH3COO- + OH-
Initial 0.125 0 0
Change -x x x
Equilibrium 0.125-x x x
Kb = x^2 / (0.125-x)
x <<1 so will ignore in denominator
1.56 X 10^-10 = x^2 / 0.125
x^2 = 0.195 X 10^-10
x = 0.442 X 10^-5 = 4.42 X 10^-6 = [OH-]
pOH = -log[OH-] = -log[4.42 X 10^-6]
pOH = 5.35
pH = 14-5.35 = 8.65
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