Question

A 0.6125 g sample of potassium iodate, KIO3, is dissolved in distilled water and made up to 250.00 cm3 in a volumetric flask. A 25.00cm3 protion of the solution is added to a n excess of acidified potassium iodide solution. The iodine formed requires 24.50 cm3 of sodium thiosulfate soltuion for titration

Answer 1

(Answer = 0.0254 )

Equation: To calculate the molarity of the sodium thiosulfate solution, we can use the following equation:

Molarity (Na2S2O3) = (Molarity (KIO3) * Volume (KIO3)) / Volume (Na2S2O3)

Explanation: We know the following values:

Molarity (KIO3) = 0.0250 M (calculated from the mass and volume of the KIO3 solution)

Volume (KIO3) = 25.00 cm3

Volume (Na2S2O3) = 24.50 cm3

Substituting these values into the equation, we get:

Molarity (Na2S2O3) = (0.0250 M * 25.00 cm3) / 24.50 cm3 = 0.0254 M

Therefore, the molarity of the sodium thiosulfate solution is 0.0254 M.

This means that there are 0.0254 moles of sodium thiosulfate in every liter of solution.