Table 2b interpretation of calibration curve 1

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Table 2b: Interpretation of Calibration Curve 1 Equation of Line Y= 10755x-0.0025 2 Conc. Of [Fe +3 ] in Test Solution 2.98*10 -5 3 Conc. Of [Fe +3 ] in Solution B 5.96*10 -4 4 Conc. Of [Fe +3 ] in Solution A 0.0119 Table 3: Analysis of Iron in K 3 Fe(C 2 O 4 ) 3 3H 2 O
1 Concentration of [Fe +3 ] in Solution A (moles/L) 0.0119 mol/ L 2 Total Volume of Solution A (mL) 100 ml 3 Moles of [Fe +3 ] in Solution A (mole) 0.00119 mol 4 MW of [Fe] (g/mole) 55.85g/1 mol 5 Weight of [Fe +3 ] in Solution A (g) .0665g 6 Weight of K 3 Fe(C 2 O 4 ) 3 3H 2 O used in Solution A (g) 1.00 g 7 Weight Percent [Fe +3 ] in K 3 Fe(C 2 O 4 ) 3 3H 2 O (g) 13.5 8 Theoretical Weight Percent of [Fe +3 ] in K 3 Fe(C 2 O 4 ) 3 3H 2 O (g) 11.4% 9 Percent Error of [Fe +3 ] 41.7% Table 4: Standardization of KMnO 4 solution 1 Weight of H 2 C 2 O 4 2H 2 O (g) 1.58 g 2 Molarity of H 2 C 2 O 4 2H 2 O Solution (M) 0.05M 3 Volume of H 2 C 2 O 4 2H 2 O used per titration (mL) 20 Ml 4 Moles of Oxalate (mole) .001 5 Moles of KMnO 4 (mole) 4.00 10 -4 Run # 1 Run # 2 Run # 3 6 Initial burette reading (mL) 0.00 Ml 19.00 ml 0 ml 7 Final burette reading (mL) 19.00 ml 38.00 ml 18.5 ml 8 Volume of KMnO 4 (mL) 19.00 ml 19.00 ml 18.5 ml 9 Molarity of KMnO 4 Solution (M) .0211 .0211 .0216
10 Average Molarity of KMnO 4 Solution (M) .0213 Table 5: Titration of Solution A 1 Volume of Solution A (mL) 20 ml 2 Average Molarity of KMnO 4 Solution (M) .0213 Run #1 Run #2 Run #3 3 Initial buret reading (mL) 19.00 ml 0.00 ml 4 Final buret reading (mL) 45.8 ml 36.00 ml 5 Volume of KMnO 4 Solution (mL) 26.8 ml 36.00 ml 6 Moles of KMnO 4 (mole) 5.71 10 -4 7.67 10 -4 7 Moles of Oxalate (mole) .00143 mol .0019 mol 8 Molarity of Oxalate (M) .0534 M .053 M 9 Average Molarity of Oxalate (M) .0532 M Table 6: Analysis of oxalate in K 3 Fe(C 2 O 4 ) 3 3H 2 O 1 Average Molarity of Oxalate (M) .0532 M 2 Total Volume of Solution A (mL) 100 ml 3 Moles of Oxalate (mole) .00532 mol 4 MW of [C 2 O 4 -2 ] ion (g/mole) 88.02 g/mol 5 Weight of Oxalate in Solution A (g) .468g 6 Actual Weight of K 3 Fe(C 2 O 4 ) 3 3H 2 O used to make Solution A (g) 1.00 g
7 Actual Weight Percent Oxalate in K 3 Fe(C 2 O 4 ) 3 3H 2 O 46.8% 8 Theoretical Weight Percent Oxalate in K 3 Fe(C 2 O 4 ) 3 3H 2 O 58.3 % 9 Percent Error of Oxalate 19.7% Discussion: Week #1: The percent yield of Potassium Ferric Oxalate from the product was 34.4 %. This number coming from the theoretical yield which is 6.28 grams of Potassium Ferric Oxalate however the actual yield from the experiment was 2.16 grams of Potassium Ferric Oxalate. The magnitude of the percent yield is low, because only 34.4% was obtain. More product could have been obtained if all measurement were more exact such as instead of having 5.03 grams of Ammonium Iron (ii) Sulfate (Fe(NH 4 ) 2 (SO 4 ) 2 *6H 2 O, having 5.00 grams exactly. Along with all the other measurements, these little differences could have an effect on the outcome of the product. However, with that also comes the time constraint, so if an unlimited amount of time was given for the procedure than the experiment could be more precise and might have a greater accuracy for the product. The observations I made during the synthesis of the complex that indicated that a reaction was occurring where the changes in colors and states. Such as when adding the Oxalic Acid (H2C2O4) to the solution it would turn yellow. Than when adding heat to the solution the

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