Calculate the number of moles of mno 4 in 2010 ml of

4. Calculate the number of moles of MnO
4
in 20.10 mL of .020
5. Calculate the number of moles of hydrogen peroxide needed to react with 20.10 mL of
0.020 M KMnO
4
6. Hydrogen Peroxide solution sold in the grocery store is 3%(by mass). Assuming a density
of 1.0 g/mL, calculate the molarity of 3.0% H
2
O
2
.

1. Measure out precisely 10 mL of 0.3% hydrogen peroxide solution from the dispensing
burette your teacher has prepared into a 250 mL Erlenmeyer Flask. Should you miss the
10.00 mL mark, just record the volume of your sample exactly.
2. Measure out approximately 10 M of 4.5 M sulfuric acid, H
2
SO
4
, solution from dispensing
burette your teacher has prepared into the flask containg the 0.3% hydrogen peroxide
solution. Caution: H
2
SO
4
is a strong acid, and should be handled with care.
3. Use a graduated cylinder to meaure out approximately 25 mL of water and add it to the
beaker as well.
4. Set up a ring stand, a burette clamp, and a burette to conduct the titration. Rinse and fill
the 50 Ml burette with 0.0200 M MnO
4
- solution. CAUTION: Handle the KMnO
solution with care; it has been mixed the H2SO4 which can cause painful burns if it
comes in contact with the skin.
4
Equations:
5H202 + @MnO4 + 6H – 5O2 + 2Mn + 8H2O
Ox: Mno4 + 8H + 5e- Mn + 4H2O
Red: H2O2 – 2H + O2 + 2e
Graphs:
Insufficient data
Post-Lab Questions: