chemistry

posted by .

So I posted this question yesterday and was told I had a few typos.... I fixed them and here is the question again... Please help me!!!

A solution of ferrous sulfate (FeSO4) is titrated with a solution of potassium permanganate in sulfuric acid. The balanced half reactions are as follows:

10FeSO4 + 5 H2SO4 --> 5 Fe2(SO4)3 + 10 H ^+ +10e^-
and 2 KMnO4 + 3 H2SO4 +10e^- --> 2 MnSO4 + K2SO4 + 8 H2O.

The gram-formula mass of FeSO4 is 151.91 g/mol, and that of KMnO4 is 158.04 g/mol.

1. What is the gram-equavalent mass of FeSo4 for this reaction?

2. What is the gram-equavalent mass of KMnO4 for this reaction?

3. If 5.35 g of KMnO4 are dissolved in
a liter of solution, what is the normality of the solution?

4. If 65.34 mL of 0.1000 N KMnO4 are required to titrate 45.28 mL of FeSO4 solution, what is the normality of the solution?

5. Carbon monoxide is detected in air samples by its reaction with diiodine pentoxide to form carbon dioxide and elemental iodine: CO + I2O5 --> CO2 + I2. Balance the equation.

  • chemistry -

    my answers so far...

    1. 151.91g FeSO4/1eq

    2. 31.608g KMnO4/1eq

    3. N=5eq/1L (not sure about this one)

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    If 26.223 mL of potassium permanganate solution is required to titrate 1.041 g of ferrous ammonium sulfate hexahydrate, { FeSO4(NH4)2So46H2O }, calculate the molarity of the KMno4 solution. and the equation the lab gave me was Mn04(-) …
  2. 11th grade ..CHEMISTRY

    This is a Quantitative Redox titration. (KMnO4) = 1.8 G.. 500 ML after the experiment we had to record the data of the 3 trials. 1. Trial - VolUme FeSO4 = 10.00 Ml - VOlume KMnO4 11.00 Ml 2. Trial - VolUme FeSO4 = 10.00 ML - VOlume …
  3. HARD chemistry

    A solution of ferrous sulfate (FeSO4) is titrated with a solution of potassium permanganate in sulfuric acid. The balanced half reactions are as follows: 10FeSO4 + 5 H2SO4 --> 5 Fe2(SO4)3 + 10 H ^+ +10e^- and 2 KMnO4 + # H2SO4 +10e^- …
  4. chemistry

    A solution of ferrous sulfate (FeSO4) is titrated with a solution of potassium permanganate in sulfuric acid. The balanced half reactions are as follows: 10FeSO4 + 5 H2SO4 --> 5 Fe2(SO4)3 + 10 H ^+ +10e^- and 2 KMnO4 + # H2SO4 +10e^- …
  5. CHEMISTRY

    1)If 36 mL of KMnO4 solution are required to oxidize 25 mL of 0.02932 M NaC204 solution, what is the concentration of the solution?
  6. chemistry

    A 3.75-G SAMPLE OF IRON ORE IS TRANSFORMED TO A SOLUTION OF IRON(II)SULFATE, FeSO4,AND THIS SOLUTION IS TITRATED WITH 0.150 M K2Cr2O7. IF IT REQUIRES 43.7 mL OF POTASSIUM DICHROMATE SOLUTION TO TITRATE THE IRON(II)SULFATE SOLUTION, …
  7. Chemistry

    7) A 3.33 g sample of iron ore is transformed into a solution of iron (II) sulfate. And this solution is titrated with 0.0150 M potassium dichromate. If it requires 41.40 mL potassium dichromate solution to titrate the FeSO4, find …
  8. Chemistry

    Help please. Am doing a past exam paper and I hit a road block with this question: Chloride in a brine solution is determined by a precipitation titration. A 10.00 mL aliquot of the solution is titrated with 15.00mL of standard 0.1182 …
  9. chemistry grade 11

    ferrous sulfate was prepared by dissolution of x grams p feso4.7H20 crystals in 500 ml water. 20 ml of this solution necessities 5 ml of 0.1mol/l kmn04 for the pink color to persist. find x
  10. Chemistry

    the lead (II) nitrate in 25.49 ml of a 0.1338M solution reacts with all of the aluminum sulfate in 25.00 ml solution. What is the molar concentration of the aluminum sulfate in the original aluminum sulfate solution?

More Similar Questions