Suppose you then make a Kool-Aid solution by dissolving the powder in an entire packet of lemon-lime Kool-Aid in 250.00 mL solution. You find the powder in a packet of lemon-lime Kool-Aid has a mass of 3.694 g. 1. In the lab you titrate 5.00 mL of the lemon-lime Kool-Aid (with 5 drops of thymol blue indicator) with your NaOH(aq) solution. The titration requires 10.90 mL of NaOH(aq). A. Determine the number of moles of NaOH(aq) required to titrate 5.00 mL of your Kool-Aid solution. B. What is the concentration of your NaOH(aq) solution?C. Determine the number of moles of NaOH(aq) that would be required to titrate 250.00 mL of your Kool-Aid solution (the entire packet). 2. In the lab you titrate 25.00 mL of the lemon-lime Kool-Aid (with KI, HCl, and starch) with 0.001000 M KIO3(aq) solution. The titration requires 10.33 mL of KIO3(aq).
A. Determine the number of moles of ascorbic acid in 25.00 mL of your Kool-Aid solution. Part 5:
B. Determine the number of moles of ascorbic acid in 250.00 mL of your Kool-Aid solution (the entire packet).C. If you titrated the entire packet of Kool-Aid, how many moles of NaOH(aq) would be neutralized in the titration due to the ascorbic acid?D. To titrate the entire packet of Kool-Aid, how many moles of NaOH(aq) would be neutralized in the titration due to the citric acid?E. Determine the number of moles of citric acid in the packet of Kool-Aid solution.