Sample of the stock solution

A 6.00-mL sample of the stock solution in #1 above was used in a titration to standardize a solution of I2(aq). [NOTE: Use of chegg.com or other “homework” site to get the answers to these questions is cheating. I wrote this prelab and I do not authorize any person paid by a so-called educational website to answer these questions for students nor post the answers on the web.] The Vitamin C sample required 38.76 mL of the I2(aq) to reach the endpoint.
(a) How many mg of Vitamin C were in the sample that was titrated?
Hint: Use your answer to #1 above.
(b) How many moles of Vitamin C were in the sample that was titrated? (MM of Vitamin C = 176.1 g/mol)
(c) How many moles of I2 must have reacted with the Vitamin C in the sample? The balanced equation for the chemical reaction between Vitamin C (C6H8O6) and I2 is: C6H8O6(aq) + I2(aq) → C6H6O6(aq) + 2 H+(aq) + 2 I-(aq)
d) What must be the molarity of the solution of I2(aq) that was used as the titrant?
Hint: Molarity is “moles of solute per liter of solution”. Consider how many mL of this solution were used, and how many moles of I2 were in it!