Calculate the pH of Strong Acid Solutions

What is the pH of the solution for (a) 0.13 M HCl, (b) 6.3 M HCl, and (c) 1.0x10^-11 M HCl?

Let's explore the pH values of different concentrations of hydrochloric acid.

Answer:

The pH of a 0.13 M HCl solution is 1.000. For a 6.3 M HCl solution, the pH depends on the presence of a weak conjugate base and its concentration.

When it comes to determining the pH of a solution of a strong acid like hydrochloric acid (HCl), it is important to consider the concentration of the acid. In the case of a 0.13 M solution of HCl, the pH is calculated to be 1.000. This is due to the complete ionization of the strong acid in water, resulting in a concentration of 0.100 M hydronium ions (H3O+).

However, for a 6.3 M HCl solution, the pH calculation becomes more complex as the presence of a weak conjugate base, such as acetate ion, needs to be taken into account. The pH of this solution will be influenced by the base ionization of the conjugate base, acetate, which is present at a concentration of 0.0500 M. This calculation involves considering the equilibrium between the acid and its conjugate base.

In the case of a very dilute solution like 1.0x10^-11 M HCl, the pH value would be extremely high due to the low concentration of hydronium ions in the solution.