1. The problem statement, all variables and given/known data Equation 1 - IO3- (aq) + 6 H+ (aq) + 5 I- (aq) -> 3 I2 (aq) + 3 H20 The iodine formed will react with the ascorbic acid. Equation 2 - C6H8O6 + I 2 -> C6H6O6 + 2 I- (aq) + 2 H+ (aq) The goal is to determine the ascorbic acid concentration (mg/mL) in a Vitamin C solution. A 10mL sample Vitamin C solution was pipetted into an Erlenmeyer flask, to which water, .5 g KL(s), 5 mL of 1M HCl solution, and 1 mL 1% starch solution was mixed thoroughly. Titration began with .0137M KIO3. To reach the endpoint indicated by the blue color of the idoine-starch complex, required 18.96 mL IO3- solution. 2. Relevant equations a. calculate the number of moles IO3- required for titration. b. Calculate the number of moles of I2 (as I3-) produced in the reaction mixture. c. Calculate the number of moles of ascorbic acid (176.14 g/mole) present in the 10-mL alquot. Calculate the molarity (M) of the ascorbic acid solution. d. Calculate the mg/mL of ascorbic acid in the solution. 3. The attempt at a solution a. I am assuming the easiest way to find the number of moles I03- required for titration is to take the 18.96 mL, convert it to L and multiply it by Molarity. But the Molarity I have known is for KIO3 (.0137M) I didn't want to run this calculation without further clarification as to whether or not this is correct. Thanks!