H 2 O 2 + MnO 4 1- = Mn 2+ + O 2 in an acidic solution With the above balanced c

Question

H2O2 + MnO41- = Mn2+ + O2 in an acidic solution

With the above balanced chemical reaction and the stoichiometric relationship between hydrogen peroxide and permanganate ion, 1.900 grams of a hydrogen peroxide solution requires 14.65 mL of a 0.02500 M solution of potassium permanganate solution to reach the equivalence point.

1. How many moles of potassium permanganate or permanganate ion are needed to reach the equivalence point?

2. After calculation of the moles of permanganate ion used to reach the equivalence point; how many moles of hydrogen peroxide were titrated?

3. From the moles of hydrogen peroxide titrated, use the molar mass of hydrogen peroxide to determine the mass of hydrogen peroxide titrated.

4. The percent by mass of a solution is defined as the mass of the solute divided by the mass of the solution x 100.
If 1.900 grams of a hydrogen peroxide solution requires 14.65 mL of a 0.02500 M solution of potassium permanganate solution to reach the equivalence point. What is the percent by mass of the hydrogen peroxide solution?

Explanation / Answer

H2O2 --> O2 + 2H+ +2e-

MnO4- + 8H+5e- -> Mn2+ + 4H2O

5 H2O2 + 2 MnO4- + 6 H+ = > 2 Mn+2 + 5 O2+ 8 H2O

b) 2 moles of the permanganate r/w 5 moles of the peroxide

mole of permanganate at the eq point = .025*14.65 /1000

= 3.66 * 10 ^ -4 moles

moles of H2O2 at the eq point = 9.15 * 10 ^ -4 ( *5/2)

mass of H2O2 = 3.1 * 10 ^ -2 grams ( * 34)

% H2O2 = 1.6 % ( / 1.900 * 100)

Related Questions

Navigate

• Browse (All)
• Browse H
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.