Calculate the pH of a 0.150 M solution of benzoic acid (C6H5CO2H) if
Ka= 6.3 x 10-5for the acid. C6H5CO2H(aq) ⇌ H+(aq) + C6C5CO2-(aq)
C6H5COOH dissociates as:
C6H5COOH -----> H+ + C6H5CO2-
0.15 0 0
0.15-x x x
Ka = [H+][C6H5CO2-]/[C6H5COOH]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((6.3*10^-5)*0.15) = 3.074*10^-3
since x is comparable c, our assumption is not correct
we need to solve this using Quadratic equation
Ka = x*x/(c-x)
6.3*10^-5 = x^2/(0.15-x)
9.45*10^-6 - 6.3*10^-5 *x = x^2
x^2 + 6.3*10^-5 *x-9.45*10^-6 = 0
This is quadratic equation (ax^2+bx+c=0)
a = 1
b = 6.3*10^-5
c = -9.45*10^-6
Roots can be found by
x = {-b + sqrt(b^2-4*a*c)}/2a
x = {-b - sqrt(b^2-4*a*c)}/2a
b^2-4*a*c = 3.78*10^-5
roots are :
x = 3.043*10^-3 and x = -3.106*10^-3
since x can't be negative, the possible value of x is
x = 3.043*10^-3
So, [H+] = x = 3.043*10^-3 M
use:
pH = -log [H+]
= -log (3.043*10^-3)
= 2.5167
Answer: 2.52
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