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A student used an acid-base titration to determine the molar mass of a solid weak monoprotic acid like $KHP$. This student titrated a weighed sample of the solid acid, after dissolving it in water in a flask, with a standardized $NaOH$ solution in a buret.

Which of the following could explain why the student obtained a molar mass that was too large?

A

Some of the solid monoprotic acid still remained on the weighing paper and was not transferred to the flask for titration.

B

More water was used to dissolve the solid monoprotic acid than what the lab called for.

C

Addition of some base beyond the endpoint of the titration.

D

The buret was not conditioned with the standardized $NaOH$ solution, but with distilled water at the beginning of the titration.

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