Wednesday
July 8, 2015

Homework Help: college chemistry

Posted by KELLY on Monday, October 4, 2010 at 12:21am.

A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Fe^2+ in acid and then titrating the Fe^2+ with MnO4^-. A 1.3510 g sample was dissolved in acid and then titrated with 39.32 mL of 0.03190 M of KMnO4. The balanced equation is:
8H^+(aq)+5Fe^2+(aq)+MnO4^-(aq)->5Fe^2+(aq)+Mn^2+(aq)+4H2O(l)
Calculate the mass percent of iron in the ore.

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

More Related Questions

Members