A student titrates permanganate (MnO4-) to acidified iron (Fe2+ (aq)) solution. The conical flask contains dissolved iron (II) to which is added sulph
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 (MnO4â) 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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Photo credit: © MARTYN F. CHILLMAID/SCIENCE PHOTO LIBRARY / Alamy / Afripics
License: Licensed
Model Released: No
Keywords: -, acid, acidic, acidified, agent, burette, conical, dissolved, fe2+, flask, gloves, ii, iron, mn2+, mno4-, molarity, nitrile, oxidizing, permanganate, point, potassium, solution, sulphuric, titrates
