Suppose a standardstrong-base solution was prepared by weighing out 1.934 g of NaOHin 500 mL of water. This solution was titrated against KHPdissolved in 200 mL of water required 48.23 mL of the basesolution.
1. Howmany 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 andthe volume of water used?

3. How many moles of KHP were weighed out?

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

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

6. Explain the difference in the answers toquestion 2 and question 5. Which is the "correct"value for the concentration of the standard NaOH solution?
A solution ofH2SO4 with unknown concentration was titratedwith the standard base described above. A volume of 5.03 mLof the acid solution required 12.07 mL of the standard base toreach the end point using phenolphthalein indicator.

7. Howmany moles of standard base were required to neutralize theH2SO4 solution?

8. How many molesof H2SO4 were present in the sample of acidtotrated?

9. What is themolarity of the acid solution?