What would be the effect on the molarity of the NaOH solution if some of the wat

Question

What would be the effect on the molarity of the NaOH solution if some of the water evaporated from the Florence flask after the NaOH solution was standardized with the KHP? (higher, lower or unchanged from the true value) Explain. What would be the effect of this on the calculated molecular weight of the add unknown? (higher, lower, or unchanged from the true value) Explain. When standardizing the base, using KHP, what would be the effect on the molarity of the NaOH solution if some of the solution was accidentally spilled in filling the buret? Is it necessary to know exactly how much water is used to dissolve the samples of KHP or the acid unknowns in each titration? Explain. Suppose some of your unknown sample has failed to dissolve even after you have titrated to your end point. What effect would this have on the calculated molecular weight of your unknown? Explain.

Explanation / Answer

1. Have you ever seen what happens to a salt solution as the water evaporates? It gets more concentrated salt solution.

1.B. If the NaOH were more concentrated that you actually thought it was, you would use Less of it to titrate the acid. Therefore the strength of the acid would be calculated to be stronger than it actually was.

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