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Suppose a standard strong-base solution was prepared by weighing out 2.514 g of NaOH in 500 mL of water. This solution was titrated against KHP to an end point established from a pH titration curve; 1.237 g of KHP dissolved in 200 mL of water required 62.699 mL of the base solution.

1. How many moles of NaOH were initially weighed out to prepare the "standard base solution?"

2. What is the apparent molarity of the "standard base," using the mass of NaOH weighed out and the volume of water used?

3. How many moles of KHP were weighed out?

4. How many moles of NaOH were required to neutralize the KHP that was weighed out?

KC8H4O4H(aq) + NaOH ? NaKC8H4O4(aq) + H2O(l)

5. What is the molarity of the "standard base"using the information obtained from KHP titration?

6. Explain the difference in the answers to question 2 and question 5. Which is the "correct" value for the concentration of the standard NaOH solution? Why?

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Category:- Chemistry
Reference No.:- M9478172

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