Question

In: Chemistry

Phenol (C6H5OH) has a Ka = 1.05 x 10-10. If 100.0 mL of a 0.5000 M...

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

CORRECT ANS: >7

Solutions

Expert Solution

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


Related Solutions

Calculate the pH of a 0.587 M aqueous solution of phenol (a weak acid) (C6H5OH, Ka...
Calculate the pH of a 0.587 M aqueous solution of phenol (a weak acid) (C6H5OH, Ka = 1.0×10-10) and the equilibrium concentrations of the weak acid and its conjugate base Calculate the pH of a 0.0183 M aqueous solution of acetylsalicylic acid (HC9H7O4, Ka = 3.4×10-4) and the equilibrium concentrations of the weak acid and its conjugate base
What is the pH of a 0.11 M solution of C6H5OH (Ka = 1.3 x 10^-10)?
What is the pH of a 0.11 M solution of C6H5OH (Ka = 1.3 x 10^-10)?
250.0 mL of 0.10 M HA (Ka = 1.0 x 10-4 ) is mixed with 100.0...
250.0 mL of 0.10 M HA (Ka = 1.0 x 10-4 ) is mixed with 100.0 mL 0.25 M KOH. What is the pH?
21. The pH of a 0.120 M phenol solution is (Ka of phenol = 1.3 x...
21. The pH of a 0.120 M phenol solution is (Ka of phenol = 1.3 x 10-10): a. 1.000 b. 10.81 c. 11.11 d. 5.40 e. 4.48 22. Which list gives equal concentrations of the following solutions in order of decreasing acidity? HC3H5O3 (Ka = 1.4 x 10-4)       H2O (Ka = 1.0 x 10-14)              HOCl (Ka = 3.5 x 10-8) HCN (Ka = 4.9 x 10-10)                HCl (Ka = 2 x 106) a. HC3H5O3 > HCl >...
What is the pH of 1.05 M Cu(NO3)2 ? Ka=3 x 10^-8 Ka is a acid.
What is the pH of 1.05 M Cu(NO3)2 ? Ka=3 x 10^-8 Ka is a acid.
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 10-5) by...
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 10-5) by 0.100 M KOH. Calculate the pH of the resulting solution after 0.0mL of KOH has been added.
Consider the titration of 100.0 mL of 1.00 M HA (Ka=1.0*10^-6) with 2.00 M NaOH. A....
Consider the titration of 100.0 mL of 1.00 M HA (Ka=1.0*10^-6) with 2.00 M NaOH. A. Determine the pH before the titration begins B. Determine the volume of 2.00 M NaOH required to reach the equivalence point C. Determine the pH after a total of 25.0 mL of 2.00 M NaOH has been added D. Determine the pH at the equivalence point of the titration. Thank you in advance!
Consider the titration of 100.0 mL of 0.016 M HOCl (Ka=3.5×10?8) with 0.0400 M NaOH. 1)...
Consider the titration of 100.0 mL of 0.016 M HOCl (Ka=3.5×10?8) with 0.0400 M NaOH. 1) How many milliliters of 0.0400 M NaOH are required to reach the equivalence point? 2) Calculate the pH after the addition of 10.0 mL of 0.0400 M NaOH. 3) Calculate the pH halfway to the equivalence point . 4) Calculate the pH at the equivalence point. thank you!
You react 100.0 mL 1.01 M HBr(aq) with 99.1 mL of 1.05 M KOH(aq) solution. How...
You react 100.0 mL 1.01 M HBr(aq) with 99.1 mL of 1.05 M KOH(aq) solution. How many moles are actually neutralized? The density of each solution is 1.04 g/mL. Cpcal = 7.0 J/oC; Cs = 4.18 J/g·oC   The DT = 6.3 oC. Calculate q and DH/mole.
25.00 mL of 0.185 M HCN (Ka = 4.90 x 10^-10) was titrated with 18.50 mL...
25.00 mL of 0.185 M HCN (Ka = 4.90 x 10^-10) was titrated with 18.50 mL of Ca(OH)2. What is the pH of the original HCN solutuon? What is the pH after 9.25 mL of base have been added?
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT