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# 1. You wish to prepare 1.0 L of 0.25 M KMnO4 from solidKMnO4. How many grams of solid KMnO4 should you use?2. You wish to prepare 1.0 L of 0.25 M KMnO4 from aconcen...

## Question

###### 1. You wish to prepare 1.0 L of 0.25 M KMnO4 from solidKMnO4. How many grams of solid KMnO4 should you use?2. You wish to prepare 1.0 L of 0.25 M KMnO4 from aconcentrated stock solution. How many mL of 1.0 M KMnO4 should youuse to prepare 1.0 L of 0.25 M KMnO4?3. You have prepared the KMnO4 solution but you are notsure the concentration of KMnO4 is exactly 0.25 M. You standardizethe solution by using a titration and the followingequation:2 KMnO4 (aq) + 5 Na2C2O4 (s) + 8 H2SO4 (aq) ðŸ¡ªK2SO4 (aq)

1. You wish to prepare 1.0 L of 0.25 M KMnO4 from solid KMnO4. How many grams of solid KMnO4 should you use? 2. You wish to prepare 1.0 L of 0.25 M KMnO4 from a concentrated stock solution. How many mL of 1.0 M KMnO4 should you use to prepare 1.0 L of 0.25 M KMnO4? 3. You have prepared the KMnO4 solution but you are not sure the concentration of KMnO4 is exactly 0.25 M. You standardize the solution by using a titration and the following equation: 2 KMnO4 (aq) + 5 Na2C2O4 (s) + 8 H2SO4 (aq) ðŸ¡ª K2SO4 (aq) + 2 MnSO4 (aq) + 10 CO2 (g) + 10 Na2SO4 (aq) + 8 H2O (l) 0.896 grams of Na2C2O4 is needed to completely react with 10.50 mL of the KMnO4. (A) Using the mass of Na2C2O4, determine the moles of Na2C2O4 used in the titration. (B) Using your answer from (A) and the mole ratio from the equation, determine the moles of KMnO4 used in the titration. (C) Using you answer from (B) and the volume of KMnO4 specified in the problem, determine the exact concentration of KMnO4.

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