If the stockroom fails to dry the KHP to remove the waters of hydration, the student's calculated concentration

for the standardized base will be:

____________ (low, high, or unaffected)
A drop of NaOH is hanging from the buret tip before the titration of KHP. Once the student begins the titration that drop falls into the KHP solution. The calculated concentration for the standardized base wil be
_____________ (low, high, or unaffected)

We prefer that you tell us your intended answers and WHY you answered that way. Otherwise, we are simply filling in the blanks for you and doing your homework.
Some tips on standardizatin with KHP.
mols KHP = mols NaOH
g/molar mass KHP = volume NaOH x M NaOH.

high, low

If the stockroom fails to dry the KHP to remove the waters of hydration, the student's calculated concentration for the standardized base will be:

Answer: high

Explanation: The presence of waters of hydration in KHP would result in an increased mass of the compound. This would lead to a higher calculated concentration of the standardized base, as the molar mass used in the calculation would be higher than the actual molar mass of KHP without hydration.

A drop of NaOH is hanging from the buret tip before the titration of KHP. Once the student begins the titration, that drop falls into the KHP solution. The calculated concentration for the standardized base will be:

Answer: low

Explanation: The drop of NaOH falling into the KHP solution before the titration will result in excess NaOH being added to the reaction mixture. This would lead to an increase in the volume of NaOH used, which would then decrease the calculated concentration of the standardized base.

If the stockroom fails to dry the KHP to remove the waters of hydration, it means that the KHP still contains water molecules. This will lead to an overestimation of the molar mass of KHP during the standardization process.

1. If the KHP is not completely dried, the calculated concentration for the standardized base will be: high

The presence of water molecules in the KHP will increase its apparent molar mass. Since the calculation of the concentration of the standardized base requires the accurate determination of the molar mass of KHP, any overestimation will result in a higher calculated concentration.

2. If a drop of NaOH falls into the KHP solution before the titration begins, the calculated concentration for the standardized base will be: unaffected

The presence of a small drop of NaOH entering the KHP solution will have a negligible effect on the overall concentration calculation. The concentration of the base will still be accurately determined by the volume of NaOH used in the titration and its molar concentration.

In summary:
1. The failure to dry the KHP (potassium hydrogen phthalate) will result in an overestimation of the calculated concentration of the standardized base, leading to a high value.
2. The drop of NaOH falling into the KHP solution before the titration will not significantly affect the accuracy of the concentration calculation, thus remaining unaffected.

The first blank is filled with "high" because if the stockroom fails to dry the KHP to remove the waters of hydration, it means that there is still water present in the KHP. Water molecules can add to the mass of the KHP, leading to an overestimation of the molar mass of KHP. Consequently, the calculated concentration for the standardized base will be higher than the actual concentration of the base.

The second blank is filled with "low" because when a drop of NaOH falls into the KHP solution before titration, it means that there is extra NaOH in the solution than what was intended. As a result, the calculated concentration for the standardized base will be lower than the actual concentration of the base.

In both cases, the calculated concentration is affected in the opposite direction of the actual concentration.