In: Chemistry
Phenol (C6H5OH) has a Ka = 1.05 x 10-10. If 100.0 mL of a 0.5000 M aqueous phenol solution is mixed with 100.0 mL of 0.5000 M aqueous sodium hydroxide, the resulting solution will have a pH |
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we have:
Molarity of C6H5OH = 0.5 M
Volume of C6H5OH = 100 mL
Molarity of NaOH = 0.5 M
Volume of NaOH = 100 mL
mol of C6H5OH = Molarity of C6H5OH * Volume of C6H5OH
mol of C6H5OH = 0.5 M * 100 mL = 50 mmol
mol of NaOH = Molarity of NaOH * Volume of NaOH
mol of NaOH = 0.5 M * 100 mL = 50 mmol
We have:
mol of C6H5OH = 50 mmol
mol of NaOH = 50 mmol
50 mmol of both will react to form C6H5O- and H2O
C6H5O- here is strong base
C6H5O- formed = 50 mmol
Volume of Solution = 100 + 100 = 200 mL
Kb of C6H5O- = Kw/Ka = 1*10^-14/1.05*10^-10 = 9.524*10^-5
concentration ofC6H5O-,c = 50 mmol/200 mL = 0.25M
C6H5O- dissociates as
C6H5O- + H2O -----> C6H5OH + OH-
0.25 0 0
0.25-x x x
Kb = [C6H5OH][OH-]/[C6H5O-]
Kb = x*x/(c-x)
Assuming small x approximation, that is lets assume that x can be ignored as compared to c
So, above expression becomes
Kb = x*x/(c)
so, x = sqrt (Kb*c)
x = sqrt ((9.524*10^-5)*0.25) = 4.88*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)
9.524*10^-5 = x^2/(0.25-x)
2.381*10^-5 - 9.524*10^-5 *x = x^2
x^2 + 9.524*10^-5 *x-2.381*10^-5 = 0
Let's solve this quadratic equation
Comparing it with general form: (ax^2+bx+c=0)
a = 1
b = 9.524*10^-5
c = -2.381*10^-5
solution of quadratic equation is found by below formula
x = {-b + √(b^2-4*a*c)}/2a
x = {-b - √(b^2-4*a*c)}/2a
b^2-4*a*c = 9.525*10^-5
putting value of d, solution can be written as:
x = {-9.524*10^-5 + √(9.525*10^-5)}/2
x = {-9.524*10^-5 - √(9.525*10^-5)}/2
solutions are :
x = 4.832*10^-3 and x = -4.927*10^-3
since x can't be negative, the possible value of x is
x = 4.832*10^-3
[OH-] = x = 4.832*10^-3 M
we have below equation to be used:
pOH = -log [OH-]
= -log (4.832*10^-3)
= 2.4
we have below equation to be used:
PH = 14 - pOH
= 14 - 2.4
= 11.7
Answer: 11.7