Question

In: Chemistry

23. A)Calculate the pH of a 0.475 M aqueous solution of hypochlorous acid (HClO, Ka =...

23.

A)Calculate the pH of a 0.475 M aqueous solution of hypochlorous acid (HClO, Ka = 3.5×10-8).
pH =

B)Calculate the pH of a 0.0354 M aqueous solution of hydrofluoric acid (HF, Ka = 7.2×10-4).
pH =

Solutions

Expert Solution

A)

HClO dissociates as:

HClO -----> H+ + ClO-

0.475 0 0

0.475-x x x

Ka = [H+][ClO-]/[HClO]

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 ((3.5*10^-8)*0.475) = 1.289*10^-4

since c is much greater than x, our assumption is correct

so, x = 1.289*10^-4 M

So, [H+] = x = 1.289*10^-4 M

use:

pH = -log [H+]

= -log (1.289*10^-4)

= 3.8896

Answer: 3.89

2)

HF dissociates as:

HF -----> H+ + F-

3.54*10^-2 0 0

3.54*10^-2-x x x

Ka = [H+][F-]/[HF]

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 ((7.2*10^-4)*3.54*10^-2) = 5.049*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)

7.2*10^-4 = x^2/(3.54*10^-2-x)

2.549*10^-5 - 7.2*10^-4 *x = x^2

x^2 + 7.2*10^-4 *x-2.549*10^-5 = 0

This is quadratic equation (ax^2+bx+c=0)

a = 1

b = 7.2*10^-4

c = -2.549*10^-5

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 = 1.025*10^-4

roots are :

x = 4.701*10^-3 and x = -5.421*10^-3

since x can't be negative, the possible value of x is

x = 4.701*10^-3

So, [H+] = x = 4.701*10^-3 M

use:

pH = -log [H+]

= -log (4.701*10^-3)

= 2.3278

Answer: 2.33


Related Solutions

Determine the percent ionization of a 0.014 M solution of hypochlorous acid, HClO. The Ka for...
Determine the percent ionization of a 0.014 M solution of hypochlorous acid, HClO. The Ka for the acid is 3.5x10^–8. A) 3.5x10 ^–6 % B) 4.9x10^–9 % C) 7.0 x 10^–3 % D) 5.0 x10^–2 % E) 1.58x 10^–1 %
Find the pH of a 0.0106 M solution of hypochlorous acid. (The value of Ka for...
Find the pH of a 0.0106 M solution of hypochlorous acid. (The value of Ka for hypochlorous acid is 2.9×10−8.) Express your answer using two decimal places.
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
Part A: Calculate the pH of a 0.316 M aqueous solution of hydrofluoric acid (HF, Ka...
Part A: Calculate the pH of a 0.316 M aqueous solution of hydrofluoric acid (HF, Ka = 7.2×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH=? [HF]equilibrium= ? [F-]equilibrium= ? Part B:Calculate the pH of a 0.0193 M aqueous solution of chloroacetic acid (CH2ClCOOH, Ka = 1.4×10-3) and the equilibrium concentrations of the weak acid and its conjugate base. pH=? [CH2ClCOOH]equilibrium = ? [CH2ClCOO- ]equilibrium = ?
Calculate the pH of a 0.449 M aqueous solution of acetylsalicylic acid (aspirin) (HC9H7O4, Ka =...
Calculate the pH of a 0.449 M aqueous solution of acetylsalicylic acid (aspirin) (HC9H7O4, Ka = 3.0×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH =    [HC9H7O4 ]equilibrium =    M [C9H7O4- ]equilibrium =    M
pH of Aqueous Sulfuric Acid Calculate the pH of a 2.07×10-3 M solution of H2SO4. (Ka...
pH of Aqueous Sulfuric Acid Calculate the pH of a 2.07×10-3 M solution of H2SO4. (Ka = 0.0120 for HSO4-)
A buffer solution is PARTIALLY neutralizing hypochlorous acid with sodium hydroxide; the Ka of HClO is...
A buffer solution is PARTIALLY neutralizing hypochlorous acid with sodium hydroxide; the Ka of HClO is 3.5 x 10-8 . Use the Henderson-Hasselbalch equation. a) If 50.0 mL of 1.00M HClO is used to make the buffer, what volume of 0.500M NaOH is needed for the final pH of the buffer to be equal to the pKa of the acid? b) Assuming no density change upon mixing, what are the concentrations of the wek acid (HClO) and its conjugate base...
22. A)The pH of an aqueous solution of 0.475 M hypochlorous acid is B)The pOH of...
22. A)The pH of an aqueous solution of 0.475 M hypochlorous acid is B)The pOH of an aqueous solution of 0.475 M formic acid, HCOOH is
Ka for hypochlorous acid, HClO, is 3.0x10-8.Calculate the pH after 10.0, 20.0, 30.0, and 40.0 mL...
Ka for hypochlorous acid, HClO, is 3.0x10-8.Calculate the pH after 10.0, 20.0, 30.0, and 40.0 mL of 0.100MNaOH have been added to 40.0 mL of 0.100 M HClO. I am mostly confused on when 40.0 mL is added, because that will be the equivalence point I believe.
1. The Ka of hypochlorous acid (HCLO) is 3.0x10-8. What is the pH at 25 C...
1. The Ka of hypochlorous acid (HCLO) is 3.0x10-8. What is the pH at 25 C of an aqueous solution that is .0200 M in HCLO? 2. A .10 M aqueous solution of the weak base B at 25 C has a pH of 8.00. The Value of Kb for B is _____.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT