Conduct a practical investigation to measure the pH of a range of acids and bases

Acid/Base Reactions > Using Brønsted–Lowry Theory >

Problem Statement: – Calculate the pH of the following solutions:

  1. 01M HCl
  2. 05M H2SO4
  3. 001M KOH

Solution:

1. pH of 0.01M HCl solution

Since HCl is a strong acid, it completely dissociates in aqueous solution

Therefore, the concentration of H+, [H+] will be 0.01M

Now, pH = – log[H+]

= – log (0.01)
= 2

2. pH of 0.05M H2SO4 solution

Since H2SO4 is a strong acid, it completely dissociates in aqueous solution

Therefore, [H+] = 0.01M

Now, pH = – log[H+]

= – log (0.1)
= 1

3. pH of 0.001M KOH solution

Since KOH is a strong base, it completely dissociates in aqueous solution

Therefore, [OH–] = 0.01M

Now, pOH = – log[OH–]

= – log (0.001)
= 3

Hence, pH = 14 – pOH = 14 –  3 = 11