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Calculate the - total number of moles of oxalate ions (sources are oxalic acid solutions and potassium oxalate monohydrate is 0.0186 moles) - total number of moles of Fe3+ ions (source is ferrous ammonium sulfate hexahydrate, FeSO4(NH4)2SO4.6H2O)

Calculate the - total number of moles of oxalate ions (sources are oxalic acid solutions and potassium oxalate monohydrate is 0.0186 moles) - total number of moles of Fe3+ ions (source is ferrous ammonium sulfate hexahydrate, FeSO4(NH4)2SO4.6H2O)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Calculate the

- total number of moles of oxalate ions (sources are oxalic acid solutions and potassium oxalate monohydrate is 0.0186 moles)

- total number of moles of Fe3+ ions (source is ferrous ammonium sulfate hexahydrate, FeSO4(NH4)2SO4.6H2O)

 

Vo)) LTE+ 00:19 I LTE1 4 ll 85% 80 Stir with a glass rod to dissolve and add 1 mL of 1.0 mol/L H2SO4aq) followed by 17 mL of deionized water Add 5.07 g of FeSO4(NH4),SO4. 6 H20 to a 100 mL beaker containing 25.0 mL of 0.80 mol/L oxalic acid Decant off the liquid to leave the precipitate in the beaker. Rinse it well with warm water and repeat the decanting. Decanting the clear solution. Fisherbrand 600mL Heat while stirring, and allow the yellow precipitate to settle. This gives an orange coloured mixture, which you need to mix well. Dissolve 3.09 g of Add this solution of potassium oxalate to your yellow precipitate. potassium oxalate in 10 mL of warm water Addition of 8.5 ml. of 0.88 M This gives you a beautiful bright green solution of your product! H202 100 mL Fill a burette Dispense 8.5 mL of the hydrogen peroxide into your orange solution while stirring, and then heat your solution to 85 -90 °C before adding 7.0 mL of 0.80 mol/L oxalic acid, followed by 1.5 mL of the hydrogen peroxide from the burette. with approximately 15 mL of 0.88 mol/L hydrogen peroxide solution Allow this to cool down to room temperature.
Transcribed Image Text:Vo)) LTE+ 00:19 I LTE1 4 ll 85% 80 Stir with a glass rod to dissolve and add 1 mL of 1.0 mol/L H2SO4aq) followed by 17 mL of deionized water Add 5.07 g of FeSO4(NH4),SO4. 6 H20 to a 100 mL beaker containing 25.0 mL of 0.80 mol/L oxalic acid Decant off the liquid to leave the precipitate in the beaker. Rinse it well with warm water and repeat the decanting. Decanting the clear solution. Fisherbrand 600mL Heat while stirring, and allow the yellow precipitate to settle. This gives an orange coloured mixture, which you need to mix well. Dissolve 3.09 g of Add this solution of potassium oxalate to your yellow precipitate. potassium oxalate in 10 mL of warm water Addition of 8.5 ml. of 0.88 M This gives you a beautiful bright green solution of your product! H202 100 mL Fill a burette Dispense 8.5 mL of the hydrogen peroxide into your orange solution while stirring, and then heat your solution to 85 -90 °C before adding 7.0 mL of 0.80 mol/L oxalic acid, followed by 1.5 mL of the hydrogen peroxide from the burette. with approximately 15 mL of 0.88 mol/L hydrogen peroxide solution Allow this to cool down to room temperature.
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