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Finding moles of iron in a sample

Finding moles of iron in a sample

C029/1117

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Credit

MARTYN F. CHILLMAID / SCIENCE PHOTO LIBRARY MARTYN F. CHILLMAID / SCIENCE PHOTO LIBRARY

Caption

A student titrates permanganate (MnO4-) to acidified iron (Fe2+ (aq)) solution. The conical flask contains dissolved iron (II) to which is added sulphuric acid to make sure the solution is acidic. The burette contains potassium permanganate (KMnO4), a strong oxidizing agent, with a known molarity. As the potassium permanganate is dripped into the flask the purplish colour disappears as permanganate (MnO4–) changes to clear manganese (Mn2+). The end point is reached when the solution turns a faint pinkish purple. The object is to ascertain the moles of iron in the sample.

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