What is the [H+] in a 0.10 M solution of ascorbic acid,C6H8O6?

Ascorbic acid = HA

................HA ==> H^+ + A^-
initial.........0.1.....0......0
change..........-x......x......x
equil..........0.1-x.....x.....x

Ka = (H^+)(A^-)/(HA)
Substitute from the ICE chart and solve for x, then convert to pH.

To find the [H+] in a 0.10 M solution of ascorbic acid (C6H8O6), we need to consider the ionization of ascorbic acid in water. Ascorbic acid, also known as Vitamin C, is a weak acid and ionizes partially in water to release hydrogen ions (H+).

The chemical equation for the ionization of ascorbic acid is as follows:

C6H8O6 + H2O ⇌ H3O+ + C6H7O6-

In this equation, C6H8O6 represents ascorbic acid, H2O is water, H3O+ is the hydronium ion, and C6H7O6- is the ascorbate ion.

Since ascorbic acid is a weak acid, it does not ionize completely in water. Instead, it partially dissociates into hydronium ions (H3O+) and ascorbate ions (C6H7O6-). Therefore, the [H+] concentration in the solution will be less than the initial concentration of ascorbic acid (0.10 M).

To find the [H+], we need to know the equilibrium constant for the ionization of ascorbic acid, which is represented by Ka. Unfortunately, the Ka value for ascorbic acid is not readily available. Without this value, we cannot calculate the [H+] accurately.

However, if we assume that the ionization is negligible, we can make an approximation. In this case, we can consider the initial concentration of ascorbic acid (0.10 M) as the [H+] concentration.

Keep in mind that this approximation may not be completely accurate, but it can give us a rough estimate of the [H+] in the solution.

Therefore, the [H+] in a 0.10 M solution of ascorbic acid is approximately 0.10 M.