A 0.108 M sample of a weak acid is 4.16% ionized in solution. what is the hydroxide concentration of this solution?

I know that i set up an ice table. The equation would be weak acid + H20 goes to OH + the acid. What do i do with the 4.16 %? How does that fit into the problem. Do i use that to figure out the Kb value?

Let's let HA stand for the weak acid.

HA + H2O ==> H3O^+ + A^-
You also know that
H2O ==> H^+ + OH^- and
Kw = (H^+)(OH^-)

So if the solution is 0.108 M and the solution is 4.16% ionized, then the (H^+)= 0.108 x 0.0416 = ??
Now use (H^+) and Kw to calculate (OH^-). Check my work.

To find the hydroxide concentration of the solution, you first need to determine the equilibrium concentration of the weak acid and its conjugate base. Then, using the percent ionization, you can calculate the concentration of the hydroxide ion.

Let's break down the steps:

Step 1: Find the equilibrium concentration of the weak acid and its conjugate base.
- Let's assume that the initial concentration of the weak acid is [HA].
- Since the weak acid is only 4.16% ionized, we can assume that the concentration of the undissociated weak acid ([HA]) is (100% - 4.16%) = 95.84% = 0.9584.
- The concentration of the conjugate base ([A-]) can be assumed to be equal to the percent ionization (4.16%) or 0.0416.

Step 2: Calculate the hydroxide concentration using the Kb value.
- You mentioned using the Kb value; however, for this problem, we don't actually need the Kb value. The Kb value is typically used to find the equilibrium constant for the hydrolysis of the weak base (conjugate base). Here, we want to find the hydroxide concentration directly.

Step 3: Determine the hydroxide concentration.
- Since the weak acid and hydroxide are in a 1:1 stoichiometric ratio according to the balanced equation, the concentration of OH- is equal to the concentration of weak acid's conjugate base ([A-]).
- Therefore, the hydroxide concentration in the solution is 0.0416 M.

So, to summarize, you can find the hydroxide concentration by assuming the initial concentrations of the weak acid and its conjugate base based on the percent ionization, and then taking the concentration of the conjugate base as the hydroxide concentration.