Question

Question 1

Calculate analytical concentration for each of the following solutions:

a) HCl solution, pH = 1.34

b) Acetic acid solution, pH = 4.31

c) Sulfuric acid solution, pH = 2.21

d) Potassium hydroxide solution, pH = 12.21

Acetic acid: pKa = 4.76

Sulfuric acid: pKa,1 = strong, pKa,2 = 1.99

In water, [H3O+][OH–] = 1.00 ! 10–14

Ignore the effect of ionic strength.

Answer 1

Calculate analytical concentrations for,

a) HCl solution

pH = -log[H+] = 1.34

[H+] = 0.0457 M

Concentration of HCl solution = 0.0457 M

b) Acetic acid solution

pH = 4.31

[H+] = 4.9 x 10^-5 M

analytical concentration [acetic acid] = (4.9 x 10^-5)^2/1.8 x 10^-5 = 1.33 x 10^-4 M

c) sulfuric acid

pH = 2.21

[H+] = 6.16 x 10^-3 M

Is the concentration = 0.00616 M

d) potassium hydoxide solution

pH = 12.21

pOH = 14 - pH = 1.79

[OH-] = 0.0162 M

Is the concentration of the solution = 0.0162 M