When standardizing an iodine solution, 30.37 ml of the solution was required to
completely oxidize 10.00 ml of a 5 mg/ml solution of ascorbic acid. what is the
molarity of the titrant?

First thing, we need to know the chemical equation for the titration reaction and it is as follows:

KIO3(aq) + 6 H+ (aq) + 5 I- (aq) = 3 I2(aq) + 3 H2O(l) + K+ (aq) 
 C6H8O6(aq) + I2(aq) = C6H6O6(aq) + 2 I- (aq) + 2 H+ (aq)

We are given the amounts and the concentrations. We use these values to calculate what is needed. We calculate as follows:

5 mg/mL C6H8O6 ( 10.0 mL ) ( 1 g / 1000 mg ) (1 mol / 176.14 g) ( 1 mol I2 / 1 mol C6H8O6 ) ( 1 mol KIO3 / 3 mol I2 ) = 9.46x10^-5 mol KIO3 needed

Molarity = 9.46x10^-5 mol KIO3 / .03037 L = 0.003 M KIO3

mention the spill to the teacher clean the area and throw the broken pieces away

explanation: