Investigating Solution Concentration Using an Oscillating Reaction

Question

You will prepare 100.00 mL of a solution with final concentration of 0.150 moles/L malonic acid solution CH2(COOH)2 and 0.0200 moles/L MnSO4

You are provided:

1. Solid malonic acid, CH2(COOH)2
2. 0.145 moles/L MnSO4 stock solution
3. Calculations for Solution B

Write in the flask the amounts of solutions and mass of solid you will add to the flask.

Answer 1

Very similar to your previous question.

For malonic acid:

molar mass CH₂(COOH)₂ = 104.1 g / mol

100.00 ml = 0.10000 L

0.150 mol / L x 0.1000 L x 104.1 g / L = 1.56 g of malonic acid needed

For MnSO₄:

(x ml)(0.145 M) = (100.00 ml)(0.0200 M)

x = 13.8 mls of 0.145 M MnSO₄ solution needed

To a 100.0 ml volumetric flask, add 1.56 g of malonic acid. Dissolve in sufficient distilled water. To this, add 13.8 mls of the 0.145 M MnSO₄ solution, and finally dilute the solution to 100.00 mls.