Question

A sample of an Iron Oxalato complex salt weighting 0.13 grams requires 32.74 mL of 0.01 M KMnO4 to turn the solution a very light pink color at the quivalence point. Calculate the number of moles of KMnO4 added.

Answer 1

Answer: The number of moles of $KMnO_4$ added are 0.0003

Explanation:

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

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in ml)}}$     .....(1)

Molarity of $KMnO_4$ solution = 0.01 M

Volume of solution = 32.74 mL

Putting values in equation 1, we get:

$0.01M=\frac{\text{Moles of }KMnO_4\times 1000}{32.67ml}\\\\\text{Moles of }KMnO_4=\frac{0.01mol/L\times 32.74}{1000}=0.0003mol$

Thus the number of moles of $KMnO_4$ added are 0.0003