Following the instructions in your lab manual, you have titrated a 25.00 mL sample of 0.0100 M KIO3 with a solution of Na2S2O3 of unknown concentration. The endpoint was observed to occur at 16.50 mL. 1. How many moles of KIO3 were titrated? Show work! 2. How many moles of Na2S2O3 did this require?

For 1: The amount of potassium iodate that were titrated is moles

For 2: The amount of sodium thiosulfate required is moles

Explanation:

To calculate the number of moles for given molarity, we use the equation:

Molarity of solution = 0.0100 M

Volume of solution = 25 mL

Putting values in above equation, we get:

Hence, the amount of potassium iodate that were titrated is moles

The chemical equation for the reaction of potassium iodate and sodium thiosulfate follows:

By Stoichiometry of the reaction:

2 moles of potassium iodate reacts with 1 mole of sodium thiosulfate

So, 0.00025 moles of potassium iodate will react with = of sodium thiosulfate

Hence, the amount of sodium thiosulfate required is moles

the answer is 1260

you spend 7 hours in school for 1 school day with 5 school days in 1 school week with 36 school weeks in a school year.

7*5*36= 1260 it's all about multiplying