In: Chemistry
Determine the [OH−] of a 0.16 M ammonia solution
Determine pH of a 0.16 M ammonia solution.
Determine pOH of a 0.16 M ammonia solution.
1)
NH3 dissociates as:
NH3 +H2O -----> NH4+ + OH-
0.16 0 0
0.16-x x x
Kb = [NH4+][OH-]/[NH3]
Kb = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Kb = x*x/(c)
so, x = sqrt (Kb*c)
x = sqrt ((1.8*10^-5)*0.16) = 1.697*10^-3
since x is comparable c, our assumption is not correct
we need to solve this using Quadratic equation
Kb = x*x/(c-x)
1.8*10^-5 = x^2/(0.16-x)
2.88*10^-6 - 1.8*10^-5 *x = x^2
x^2 + 1.8*10^-5 *x-2.88*10^-6 = 0
This is quadratic equation (ax^2+bx+c=0)
a = 1
b = 1.8*10^-5
c = -2.88*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 = 1.152*10^-5
roots are :
x = 1.688*10^-3 and x = -1.706*10^-3
since x can't be negative, the possible value of x is
x = 1.688*10^-3
so,
[OH-] = x = 1.688*10^-3 M
Answer: 1.7*10^-3 M
2 and 3)
use:
pOH = -log [OH-]
= -log (1.688*10^-3)
= 2.7726
use:
PH = 14 - pOH
= 14 - 2.7726
= 11.2274
Answer:
pH = 11.2
pOH = 2.8