[elle1019]

Part one:
A volume of 50.0 mL of aqueous potassium hydroxide was titrated against a standard solution of sulfuric acid. What was the molarity of the \rm KOH solution if 19.2 mL of 1.50 M H2SO4 was needed? The equation is

2KOH(aq) +H2SO4(aq) -> K2SO4 (aq)+2H2O(l)
Express the molar concentration numerically.

Part two:
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction:

2 KMnO4(aq)+ H2O2(aq)+3 H2SO4(aq) -> O2(g)+2 MnSO4(aq)+K2SO4 (aq)+4 H2O(l)

A certain amount of hydrogen peroxide was dissolved in 100.mL of water and then titrated with 1.68 M KMnO4. How much H2O2 was dissolved if the titration required 12.8 mL of the KMnO4 solution?

Thank you for any help,
much appriciated!

[sjb]

Part one:
A volume of 50.0 mL of aqueous potassium hydroxide was titrated against a standard solution of sulfuric acid. What was the molarity of the \rm KOH solution if 19.2 mL of 1.50 M H2SO4 was needed? The equation is

2KOH(aq) +H2SO4(aq) -> K2SO4 (aq)+2H2O(l)
Express the molar concentration numerically.

How many moles of sulfuric acid did you consume during the titration?