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Suppose, in an experiment to determine the amount of sodium hypochlorite in bleach, you titrated a 23.92 mL sample of 0.0100 M K I O 3 with a solution of N a 2 S 2 O 3 of unknown concentration. The endpoint was observed to occur at 13.80 mL . How many moles of K I O 3 were titrated

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Answer:

2.39x10⁻⁎ moles

Explanation:

As the problem asks us the number of moles of KIO₃ that were titrated, all that is required of us is to calculate how many moles of KIO₃ are there in 23.92 mL of a 0.0100 M solution (All moles in the samples are titrated).

We can do so by using the definition of molarity:

  • Molarity = moles / liters

converting 23.92 mL ⇒ 23.92 / 1000 = 0.02392 L

  • moles = 0.0100 M * 0.02392 L
  • moles = 2.39x10⁻⁎ moles

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