A 5.00 mL sample of vinegar, a solution of acetic acid, is titrated with 0.756 M calcium hydroxide. 10.23 mL of the calcium hydroxide is required to reach the equivalence point. What is the molarity of the acetic acid in the vinegar.

3.09 M

Explanation:

The reaction that takes place is:

First we calculate how many Ca(OH)₂ moles reacted, using the given volume and concentration:

Then we convert Ca(OH)₂ mmoles into mmoles of acetic acid, using the stoichiometric coefficients of the balanced reaction:

Finally we calculate the molarity of acetic acid, using the number of moles and given volume:

it is a good conductor

explanation:

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