• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

PPA1 Preparation of Potassium Trioxalatoferrate

Extracts from this document...


Unit 1 PPA 1: Preparation of Potassium Trioxalatoferrate Aim: The aim of the investigation was to prepare Potassium Trioxalatoferrate (III) from Ammonium Sulphate and then calculate the percentage yield. Introduction a) Ligand The oxalate ion can act as a ligand as it binds to a central metal ion to form a complex ion by the donation of one or more electron pairs into unfilled metal orbitals. In this case three negatively charged oxalate ions surround one positively charged Fe3+. The three oxalate ions attach themselves to the Fe3+ at six points creating an octahedral shape. This results in the metal complex having a net total charge of -3. b) Potassium Trioxalatoferrate http://upload.wikimedia.org/wikipedia/commons/thumb/3/33/Potassium-ferrioxalate-2D.png/250px-Potassium-ferrioxalate-2D.png 07/03/10 c) Relevant Equations Step 1: (NH4)2Fe(SO4)2.6H2O + H2C2O4 --> FeC2O4 + H2SO4 + (NH4)HSO4 +6H20 Step 2: 6FeC2O4 + 3H2O2 + 6K2C2O4 --> 4K3[Fe(C2O4)3] + 2Fe(OH)3 Step 3: 2Fe(OH)3 + 3H2C2O4 +3K2C2O4 --> 2K3(Fe(C2O4)3) ...read more.


ions to iron (III) ions. Procedure * A 100 cm3 glass beaker was weighed and approximately 5g hydrated ammonium iron(II) sulphate was added. The beaker and its contents were then reweighed. * Approximately 15 cm3 and 1 cm3 sulphuric acid were added to the ammonium iron(II) sulphate. The mixture was then warmed to dissolve the solid * After the ammonium iron(II) sulphate was dissolved 25 cm3 oxalic acid was added. (NH4)2Fe(SO4)2.6H2O + H2C2O4 --> FeC2O4 + H2SO4 + (NH4)HSO4 +6H20 Green --> Yellow * The beaker was then placed on a hot plate and slowly heated and stirred until it boiled. * The beaker was removed from the heat in order to allow the precipitate (Iron (II) Oxalate) to form at the bottom of the beaker. * The liquid was then decanted and 50 cm3 of deionised water was added to the remaining precipitate. ...read more.


* The crystals were weighed in a clock glass and then covered with filter paper and retuned to the cupboard. * Once dry, the crystals and clock were reweighed. * The percentage yield of hydrated Potassium Trioxalatoferrate was calculated. Hazards Eye protection was worn and if any chemicals were splashed onto skin it was washed off immediately. Cation was taken at all times to wear the safety equipment provided, in this case safety goggles and latex gloves. Name Hazard Hydrated Ammonium Iron (II) Sulphate Harmful if ingested and may irritate eyes Oxalic Acid Harmful if ingested and irritating to eyes and skin Potassium Oxalate Solution Harmful if ingested and irritating to eyes and skin Potassium Trioxalatoferrate Harmful if ingested and irritating to eyes and skin "20 Volume" Hydrogen Peroxide Irritating to eyes and skin Ethanol Harmful if ingested and irritating to eyes and skin, volatile, highly flammable Dilute Sulphuric Acid Corrosive ?? ?? ?? ?? ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Inorganic Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    If I didn't swirl the solution then the area in the middle of the conical flask where the sulfuric acid was falling would turn pink first as the OH- particles and H+ particles in that part of the solution would have reacted.

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    Filling the burette before each titration up to 0cm3 will avoid any mistake in calculating the difference between the two graduation marks after each titration, so the results will be all from 0, so will be more reliable because fewer calculations have been done.

  1. effects Concentration and Temperature on the Rate of Reaction

    Temperature of Reactants (K) 1/Temperature (K -1) Reaction Rate (s-1) Log To The Base e Of Reaction Rate 10 283 0.00353 0.0097 -4.636 15 288 0.00347 0.0149 -4.206 20 293 0.00341 0.0234 -3.755 25 298 0.00336 0.0353 -3.344 30 303 0.00330 0.0512 -2.972 35 308 0.00325 0.0846 -2.469 40 313

  2. determination of the percentage of oxalate in iron (II) oxalate by redox titration

    15) A few drops of standard potassium manganate (VII) solution was run out from the burette to the solution inside the conical flask with constant swirling until the solution became clear.. 16) Standard potassium manganate (VII) solution was run out from the burette to the solution inside the conical flask until the solution change from pale yellow to permangent pale pink.

  1. The preparation, analysis, and reactions of an ethanedioate complex of iron

    The solid was allowed to air dry by suction. The weight of the dry solid was weighed and the yield was calculated. Procedure for Analysis (a)Oxidation with permanganate Two portions of 0.38g of the sample complexes were added into two conical flasks separately. Each sample was dissolved in 10cm3 of water and 15cm3 of dilute sulphuric acid.

  2. Aim; 1)To prepare a standard potassium dichromate solution 2)To standardize the ammonium iron(II) sulphate ...

    (in Conical flask): 25.0cm3 of Hydrogen Peroxide Solution Indicator used: Potassium Permanganate Solution Colour of indicator changed from: Colourless to Pink Titration No. 1(trial) 2 3 4 Final burette reading (cm3) 21.40 42.60 21.30 42.50 Initial burette reading (cm3) 0.00 24.40 0.00 21.30 Volume of titrant used (cm3)

  1. Chemistry Iodine Clock

    This ensures that the solution is mixed properly. 10- Write on the flask the name of solution, that way you won't get mixed up when you make other solutions. Standard solution of Potassium Iodide We need to calculate how many moles we need. This can be worked out by this equation: Number of moles = concentration x volume

  2. Aim To study the effect of concentration of iodide ion ...

    % 0.1000 � 0.1000% 0.9000 � 0.0111% Table 1.3 Uncertainties due to dilution of KI solution *The uncertainties due to preparation of solutions are minimal and assumed to be negligible. Uncertainty due to pipette = � ?"?3 x 100 = � 0.12% # "??

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work