Investigating Solution Concentration Using an Oscillating Reaction

Question

You will prepare 50.00 mL of a solution with final concentrations of 0.200 mole/L KIO3 and 0.0800 mol/L H2SO4 You are provided: • Solid potassium iodate, KIO3 • 0.625 moles/L H2SO4 stock solution.

Calculations for Solution A?

Answer 1

Assuming both the KIO₃ and H₂SO₄ go into the same solution (solution A), you would proceed as follows:

molar mass KIO₃ = 214 g / mol

50.00 ml = 0.05000 L

0.200 mol KIO₃ / L x 0.05000 L x 214 g / mol = 2.14 g KIO₃ needed

For H₂SO₄: (x ml)(0.625 M) = (50 ml)(0.0800 M)

x = 6.4 mls of 0.625 M H₂SO₄ needed

Weigh out 2.14 g KIO₃. Place in a 50.00 ml volumetric flask. Dissolve in sufficient distilled water. Add 6.40 mls of 0.625 M H₂SO₄, and dilute solution to a final volume of 50.00 mls.