a 23.74 ml volume of .0981 M NaOH was used to titrate 25 mL of a weak monoprotic acid solution to the stoichiometric point. determine the molar concentration of the weak acid solution. Express your answer to the correct number of significant figures.
To determine the molar concentration of the weak acid solution, we need to use the concept of stoichiometry and the volume and molarity of the NaOH solution used for the titration.
Given:
Volume of NaOH solution used = 23.74 ml
Molarity of NaOH solution used = 0.0981 M
Volume of weak acid solution titrated = 25 mL
The balanced chemical equation for the reaction between NaOH and the weak acid is as follows:
NaOH + HX → NaX + H2O
From the balanced equation, we can see that the stoichiometric ratio between NaOH and HX (the weak acid) is 1:1. This means that the mole ratio between the reactants is 1:1.
To calculate the molar concentration of the weak acid solution, we can use the following formula:
Molar concentration of weak acid solution = (Volume of NaOH solution used × Molarity of NaOH solution used) / Volume of weak acid solution titrated
Substituting the given values into the formula:
Molar concentration of weak acid solution = (23.74 ml × 0.0981 M) / 25 ml
Now, let's calculate the result:
Molar concentration of weak acid solution = 0.0925 M (rounded to the correct number of significant figures)
Therefore, the molar concentration of the weak acid solution is 0.0925 M.