HA is an acid that ionizes in 10% in solution. what is the [h+] of a 0.01 m solution of ha?
4565
To determine the concentration of H+ ions in a solution of HA, we need to use the ionization constant (Ka) of the acid, as well as its initial concentration.
Given the information that HA ionizes to 10%, we can assume that only 10% of the initial concentration of HA will dissociate into H+ ions and its conjugate base (A-). This means that the remaining 90% will remain undissociated as HA.
Let's break down the steps to find the [H+] concentration:
1. Write down the chemical reaction representing the ionization of HA:
HA ⇌ H+ + A-
2. Write down the equilibrium expression using the ionization constant (Ka):
Ka = [H+][A-] / [HA]
3. Since only 10% of HA has ionized, we can write the initial concentrations as follows:
[HA] = 0.01 M (initial concentration)
[H+] = x (unknown concentration)
[A-] = x (equal to [H+] due to the 1:1 ratio in the reaction)
4. Substitute the concentrations into the equilibrium expression:
Ka = (x)(x) / (0.01 - x)
5. Since the value of Ka is not provided, we cannot calculate [H+] directly. However, we can make an assumption based on the degree of ionization given in the question. If HA ionizes to 10%, we can assume that x (the concentration of [H+]) will also be approximately 10% of the initial concentration of HA. Therefore, x ≈ 0.1(0.01) = 0.001 M.
Keep in mind that this assumption only holds true when the degree of ionization is relatively low. If the degree of ionization is high or the assumption is not valid, we would need a more accurate value of Ka to calculate [H+].
So, the approximate [H+] concentration in the 0.01 M solution of HA would be 0.001 M.
I assume you mean 0.01 M and not 0.01 m.
0.01 x 0.1 = ?