To a 25.00 ml volumetric flask, a lab technician adds a 0.150 g sample of a weak monoprotic acid, ha , and dilutes to the mark with distilled water. the technician then titrates this weak acid solution with 0.0969 m koh . she reaches the endpoint after adding 43.81 ml of the koh solution. determine the number of moles of the weak acid in the solution.

The number of moles of weak acid is moles.

Explanation:

To calculate the moles of KOH, we use the equation:

We are given:

Volume of solution = 43.81 mL = 0.04381 L      (Conversion factor: 1L = 1000 mL)

Molarity of the solution = 0.0969 moles/ L

Putting values in above equation, we get:

The chemical reaction of weak monoprotic acid and KOH follows the equation:

By Stoichiometry of the reaction:

1 mole of KOH reacts with 1 mole of weak monoprotic acid.

So, of KOH will react with = of weak monoprotic acid.

Hence, the number of moles of weak acid is moles.

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