You are titrating an unknown weak acid you hope to identify. Your titrant is a 0.0935 mol/L NaOH solution, and the titration requires 22.3 mL to reach the equivalence point. How many moles of acid were in your sample?

moles NaOH = M x L.

moles weak acid = moles NaOH IF the weak acid is a monoprotic acid; otherwise, moles acid will be 1/2 if diprotic (and both hydrogens are titrated together) or 1/3 if triprotic (and all three hydrogens are titrated together).

So dumb bob what the ans.

0.456

To determine the number of moles of acid in your sample, we can use the concept of stoichiometry and the volume and concentration of the titrant used.

The balanced chemical equation for the neutralization reaction between the weak acid and NaOH is:

Weak Acid + NaOH → Salt + Water

From the balanced equation, we can see that the mole ratio between the weak acid and NaOH is 1:1. This means that for every mole of weak acid, we need one mole of NaOH to reach the equivalence point.

Given:
- Concentration of NaOH (Titrant) = 0.0935 mol/L
- Volume of NaOH used = 22.3 mL = 0.0223 L

Now, we can calculate the number of moles of NaOH used in the titration:

Moles of NaOH = Concentration × Volume
Moles of NaOH = 0.0935 mol/L × 0.0223 L

Next, we use stoichiometry to find the number of moles of weak acid:

Moles of Weak Acid = Moles of NaOH

Since the mole ratio between the weak acid and NaOH is 1:1, the number of moles of weak acid is the same as the number of moles of NaOH used in the titration. Therefore:

Moles of Weak Acid = 0.0935 mol/L × 0.0223 L

Calculating this expression will give you the number of moles of acid in your sample.