# Chem

Suppose 22.93mL of KMnO4 solution used in the question above (KMnO4 solution in above question 36.00mL and concentration of 0.02036M)are needed to oxidize Fe(2+) to Fe(3+) in a 0.4927g pill. What is the mass percent of FeSO4 (dot) 7H2O (molar mass 278.03g/mol) in the pill?

What I would do is take the concentration of KMnO4 and then using the 22.93mL find the mols and then divide the 0.4927g by them. This gives me the molar mass of the pill. Then i find the percent by dividing the molar mass of FeSO4 (dot) H2O by the pill molar mass to find the percent. Is that correct?

Thank you :)

1. 👍 0
2. 👎 0
3. 👁 59
asked by Meso

## Similar Questions

1. ### mass percent

Suppose 22.93mL of KMnO4 solution used in the question above (KMnO4 solution in above question had concentration of 0.02036M)are needed to oxidize Fe(2+) to Fe(3+) in a 0.4927g pill. What is the mass percent of FeSO4*7H2O (molar

asked by Meso on May 22, 2011
2. ### Chemistry HELP!

In order to standardize a KMnO4 solution, 0.3498 g Na2C2O4 was dissolved in 30 mL water and 15 mL 3.0 M H2SO4. The KMnO4 solution was added to the Na2C2O4 solution until a pale pink color persisted. The titration took 29.5 mL of

asked by Prue on May 6, 2013
3. ### Chemistry HELP!

In order to standardize a KMnO4 solution, 0.3498 g Na2C2O4 was dissolved in 30 mL water and 15 mL 3.0 M H2SO4. The KMnO4 solution was added to the Na2C2O4 solution until a pale pink color persisted. The titration took 29.5 mL of

asked by Prue on May 6, 2013
4. ### Chemistry

If 36.00 mL of KMnO4 solution are required to oxidize 25.00mL of 0.02932 M Na2C2O4 solution what is the concentration of KMnO4?

asked by Tilly on November 2, 2010
5. ### Chemistry College Level

Ok, so here's my question: If exactly 14.563 grams of KMnO4 were dissolved to yield 750 mL of solution waht would be the normality of the KMnO4? From a previous question (that this question says to refer to) we have: MnO4- +8H+

asked by Tichele on April 17, 2011
6. ### Chemistry (Titrations)

In order to standardize a KMnO4 solution, 0.2848 g Fe(NH4)2(SO4)2·6H2O was dissolved in 25 mL 0.18 M H2SO4. The KMnO4 solution was added to the Fe(NH4)2(SO4)2·6H2O solution until a pale pink color persisted. The titration took

asked by Bill on November 30, 2014
7. ### chemistry

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

asked by amy on January 5, 2010
8. ### 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 -

asked by Komal on November 5, 2008
9. ### AP Chem

A solution of hydrogen peroxide, H2O2, is titrated with a solution of potassium permanganate, KMnO4. It requires 51.7 mL of 0.145 M KMnO4 to titrate 20.0 g of the solution of hydrogen peroxide. What is the mass percentage of H2O2

asked by Anna on November 3, 2008
10. ### Chemistry

A solution of hydrogen peroxide, H2O2 , is titrated with potassium permanganate, KMnO4 , according to the following equation: 5 H2O2 + 2 KMnO4+ 3H2SO4 -> 5O2 + 2 MnSO4 +8H2O + K2SO4 It requires 46.9mL of 0.145 mol/L KMnO4 to

asked by Brenan on March 30, 2008

More Similar Questions