1.00g of K3[Fe(C2O4)3] (Molar mass 437.25g/mol) Mixed with 20ml .984M sulfuric acid. TItrated with 13.4ml .028MKmNO4...

1.00g of K3[Fe(C2O4)3] (Molar mass 437.25g/mol)

Mixed with 20ml .984M sulfuric acid.

TItrated with 13.4ml .028MKmNO4

-----

What is

Moles of KMnO4 reduced?

Moles of C2O42 oxidized?

Mass of C2O42 oxidized?

Actual weight % C2O42 in KTOF3

Theoritical weight % of C2O42 in KTOF3

%Error of weight % of C2O42 in KTOF3

Expert Solution

queen_honey_blossom answered 2 years ago

Redox titration of oxalate 1.00g of K3[Fe(C2O4)3] (Molar mass 437.25g/mol) Mixed with 20ml .984M sulfuric acid....

Redox titration of oxalate 1.00g of K3[Fe(C2O4)3] (Molar mass 437.25g/mol) Mixed with 20ml .984M sulfuric acid. TItrated with 13.4ml .028MKmNO4 ----- What is Moles of KMnO4 reduced? Moles of C2O42 oxidized? Mass of C2O42 oxidized? Actual weight % C2O42 in KTOF3 Theoritical weight % of C2O42 in KTOF3 %Error of weight % of C2O42 in KTOF3

Please find the theoretical percent of Fe in K3[Fe(C2O4)3] x 3H2O Here is some information I...

Please find the theoretical percent of Fe in K3[Fe(C2O4)3] x 3H2O Here is some information I already found: Concentration of Solution A .02096 M Total Volume of Solution A .2 L Moles of Fe 4.192 x 10-3 mol Molecular Weight of Fe 55.847 g/mol Mass of Fe in Solution A .234110624 g Mass of K3[Fe(C2O4)3] x 3H2O in Solution A .93 g Weight Percent in K3[Fe(C2O4)3] x 3H2O 25.17318537634409% Theoretical % Fe in K3[Fe(C2O4)3] x 3H2O ??????? Percent Error ???????

Ethanol, C2H5OH (molar mass = 46 g/mol) is mixed with methanol, CH3OH (molar mass = 32...

Ethanol, C2H5OH (molar mass = 46 g/mol) is mixed with methanol, CH3OH (molar mass = 32 g/mol) to make an ideal solution at a given temperature. If 5.00 g of ethanol and methanol are mixed, what is the resulting vapor pressure of the solution? (the vapor pressure at the same temperature for pure ethanol is 44.5 mm Hg and pure methanol is 88.7 mm Hg)

What mass of a weak acid with a molar mass of 100 g/mol is necessary to...

What mass of a weak acid with a molar mass of 100 g/mol is necessary to neutralize 25 ml of 0.10 M NaOH solution? What is the pH of 0.15 g of sodium acetate NaC2H3O2 in 100 ml water H2O?

What mass (in g) of iron (Fe, molar mass = 55.85 g∙mol–1) is needed to experimentally...

What mass (in g) of iron (Fe, molar mass = 55.85 g∙mol–1) is needed to experimentally produce 50.0 g of iron(III) oxide (Fe2O3, molar mass = 159.70 g∙mol–1) in excess oxygen if the percent yield is 78.7%? 4Fe(s) + 3O2(g)2Fe2O3(s) A. 22.2 g B. 27.5 g C. 35.0 g D. 44.4 g

A 0.520 g sample of a diprotic acid with a molar mass of 255.8 g/mol is...

A 0.520 g sample of a diprotic acid with a molar mass of 255.8 g/mol is dissolved in water to a total volume of 23.0 mL . The solution is then titrated with a saturated calcium hydroxide solution. a. Assuming that the pKa values for each ionization step are sufficiently different to see two equivalence points, determine the volume of added base for the first and second equivalence points. b. The pH after adding 23.0 mL of the base was...

1) if you have 8.00M sulfuric acid solution, and you took 20ml of this stock solution...

1) if you have 8.00M sulfuric acid solution, and you took 20ml of this stock solution and diluted to 500mL total, what is the concentration of the dilute solution? discuss your steps when you give the answer 2) If you have 8.00M of sulfuric acid solution and you want to dilute to 400mL diluted solution with concentration of 2.0M; what volume of the stock solution you should use? what volume of solvent you need to add when you dilute it

1a) if you have 8.00M sulfuric acid solution, and you took 20ml of this stock solution...

1a) if you have 8.00M sulfuric acid solution, and you took 20ml of this stock solution and diluted to 500mL total, what is the concentration of the dilute solution? discuss your steps when you give the answer 1b) now, If you have 8.00M of sulfuric acid solution and you want to dilute to 400mL diluted solution with concentration of 2.0M; what volume of the stock solution you should use? what volume of solvent you need to add when you dilute...

Concentrated sulfuric acid is 96.0% (w/w) sulfuric acid (H2SO4, MW = 98.1g/mol) and has a density...

Concentrated sulfuric acid is 96.0% (w/w) sulfuric acid (H2SO4, MW = 98.1g/mol) and has a density of 1.84 g/mL. Determine the volume needed to prepare 500 mL of a 1.00 M solution.

Chem Question - Gases Molar Mass N = 14.01 g/mol Molar Mass H2O = 18.016 g/mol...

Chem Question - Gases Molar Mass N = 14.01 g/mol Molar Mass H2O = 18.016 g/mol Vapor Pressure of Water at 25 C is 23.76 torr Vapor Pressure of Water at 65 C is 187.54 torr (Show all work and calculations, include units in answer. If calculations must be used in several parts, rounding should be made to 6 decimal points to ensure accuracy. Final Answers can be rounded to 3 decimal points.) A syringe filled with air can be...

Question