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The Estimation of Iron (II) and Iron (III) in a Mixture Containing Both.

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A2 - The Estimation of Iron (II) and Iron (III) in a Mixture Containing Both Planning:- Fe2+ Fe3+ + e- (multiply by 5) MnO4- + 5e- + 8H+ Mn2+ + 4H2O MnO4- + 8H+ + 5Fe2+ Mn2+ + 5Fe3+ + 4H2O Background Knowledge - Iron, Fe, is a transition metal with the atomic number 26. Iron is a magnetic, malleable and metallic silver element. Iron has the ability of having multi valences, commonly Fe2+ or Fe3+. Fe2+ forms ferrous compounds, whereas Fe3+ tends to form ferric compounds. Iron can be used as a catalyst due to its multiple valances, e.g. it is used in the manufacturing of Ammonia in the Haber process. An oxidising agent will convert Iron(II) into Iron(III), the iron will lose an electron. A reducing agent will convert Iron(III) into Iron(II), the iron will gain an electron. Iron sulphate (FeSO4), also known as vitriol or copperas, is an important iron (II) compound as it forms pale green crystals containing seven molecules of water of hydration. It is mainly formed as a by - product in the pickling of iron. It can be used as a mordant in dyeing, tonics in medicines and also in the manufacturing of ink and pigments. Iron (III) compounds also have many uses, such as iron (III) oxide being used as a pigment, known as iron red, or the compound is also used as a polishing abrasive, known as rouge. ...read more.


Once cleaned, you must pipette 25cm3 of the iron solution into the conical flask. You must touch the end of the pipette on the conical flask to maintain accuracy throughout the experiment. o Into the conical flask you must add roughly 20cm3 of sulphuric acid as acidified acidic solution is the requirements for which this reaction may take place. o Fill the burette with KMnO4 using the burette filler, but be sure to remove the funnel as drops later on in the experiment may ruin results. o Now you are setup to begin titrating. Allow the potassium permanganate to flow into the titre until a permanent colour change from colourless to pink has occurred. This is your rough titration. Record your value of your burette and fill in the table below. o Repeat this procedure until you have concurrent titre volume readings i.e. your values must be within 0.1cm3 of each other. But, this time, allow the KMnO4 to flow into the solution until you are near the value you received for your rough titre. At this point you must drip the KMnO4 into the solution in the conical flask to increase the accuracy of your readings. o Throughout the whole period of titrating, you must constantly be swirling the conical flask to make sure that the colour change is permanent. o Keep all the conical flask solutions as they will be used in titration 2. ...read more.


in solution = Moles x RFM = (8.0 x 10-4).W x 55.8 = 4.5 x 10-2.W g ( Q ) Overall, the mass of Iron (III) present is the difference between the mass of Iron (II) in titration 2 and titration 1: = H - D = ( 4.5 x 10-2 )( W - V ) g ( Z ) Percentage Composition: Iron (II) : ( Mass of Iron (II) in titration 1 / Mass of Iron (II) in titration 2 ) x 100 = P / H x 100 Iron (III) : ( Mass of Iron (III) / Mass of Iron (II) in titration 2 ) x 100 = Q / H x 100 Safety * Goggles must be worn at all times while working with chemicals. * Lab coats must be worn at all times potassium permanganate stains clothes. * Wear gloves when handling sulphuric acid as it is corrosive and toxic. * Safety fillers must be used when using pipettes. * If any chemical comes into contact with your skin, you must immediately wash the area thoroughly. * Glass equipment must be handled carefully as breakages are possible. in the event of a cut, it should be seen to before continuing the practical. Sources * Chemistry in Context Fourth Edition - Graham Hill and John Holman * Microsoft Encarta 2000 Encyclopedia * Chemistry 2 textbook - OCR * Compton's Encyclopedia 2001 Edition Jaimal B Amin A2 Practical Exp 9 Mr. Latif ...read more.

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