Final answer:
For a solution with a pH of 1.3, the concentration of hydronium ions [H3O+] is calculated to be 5.01 × 10^-2 M, and the concentration of hydroxide ions [OH-] is 1.99 × 10^-13 M.
Step-by-step explanation:
Calculating [H3O+] and [OH-] for a Solution with pH = 1.3
The pH scale is a measure of the acidity or basicity of an aqueous solution. It is directly related to the concentration of hydronium ions [H3O+] with pH = -log[H3O+]. For a solution with a pH of 1.3, the concentration of hydronium ions can be calculated using this formula:
[H3O+] = 10-pH
= 10-1.3
= 5.01 × 10-2 M
Since the product of the concentrations of the hydronium and hydroxide ions is always equal to 1.0 × 10-14 at 25°C (the ion-product constant for water, Kw), we can calculate the concentration of hydroxide ions [OH-] as follows:
[OH-] = Kw / [H3O+]
= 1.0 × 10-14 / 5.01 × 10-2 M
= 1.99 × 10-13 M
Therefore, for a solution with a pH of 1.3, the concentration of hydronium ions [H3O+] is 5.01 × 10-2 M and the concentration of hydroxide ions [OH-] is 1.99 × 10-13 M.