Consider the redox titration of Fe2+ with KMnO4 as performed in 3. If 22.65 mL of...
Consider the redox titration of Fe2+ with KMnO4 as performed in 3. If 22.65 mL of a 0.02024 M KMnO4 solution was required to titrate the Fe2+ in an unknown sample that weighed 1.1243 g, what is the %Fe in the unknown?
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Consider the redox titration of Fe2+ with KMnO4 as performed in
3. If 22.65 mL of...
suppose you have an unknown sample containing Fe^2+, and you titrate it with KMnO4 standard solution....
suppose you have an unknown sample containing Fe^2+, and you
titrate it with KMnO4 standard solution. Calculate the percent of
Fe in your sample.
equation: MnO4- + 5Fe^2+ + 8H^+ --> Mn^2+ + 5Fe^3+ +
4H2O
Suppose you have an unknown sample containing Feat, and you titrate it with a KMnO4 standard solution. Calculate the percentage of Fe in your sample. Equation: MnO(+5Fe2+ + 8H - Mn2+ + 5Fe3+ + 4H20 Data 0.08124M 2.49g Molarity of the KMnO4 standard solution:...
In a redox titration, 12.52 mL of a 0.3264 M KMnO4 solution were required to titrate...
In a redox titration, 12.52 mL of a 0.3264 M KMnO4 solution were required to titrate 1.7832 g of a reducing agent ("X"). If the reducing agent undergoes a 3-electron change per formula unit: a) write the two ionic half reaction and the balanced net ionic equation. ionic MnO4-: ionic reducing agent: net ionic: b. Calculate the molar mass of the reducing agent.
The Fe2+ (55.845 g/mol) content of a 2.264 g steel sample dissolved in 50.00 mL of...
The Fe2+ (55.845 g/mol) content of a 2.264 g steel sample dissolved in 50.00 mL of an acidic solution was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 44.82 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per gram of steel Mn2+5 Fe34 H20 + 5 Fe2+ MnO8 H concentration g Fe/g steel A 1.969 g...
• CIU TEXAS INSTRUM 2. A 50.00 ml sample of solution containing Fe?ions is titrated with a 0.0216 M KMnO4 solution....
• CIU TEXAS INSTRUM 2. A 50.00 ml sample of solution containing Fe?ions is titrated with a 0.0216 M KMnO4 solution. It required 20.62 ml of the KMnO4 solution to oxidize all the Fe? ions to Fe ions by the reaction: MnO4 (aq) + Fe? ) -------> Mn(ed) Felco (unbalanced) a) What was the concentration of Fel.ions in the sample solution? b) What volume of 0.0150 M K2Cr2O7 solution would it take to do the same titration? The reaction is:...
The iron content of iron ore can be determined by titration with a standard KMnO4 solution....
The iron content of iron ore can be determined by titration with a standard KMnO4 solution. The iron ore is dissolved in HCl, and all the iron is reduced to Fe2+ ions. This solution is then titrated with KMnO4 solution, producing Fe3+ and Mn2+ ions in acidic solution. If it required 29.83 mL of 0.0447 M KMnO4 to titrate a solution made from 1.128 g of iron ore, what is the mass percent of iron in the iron ore? Mass...
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a...
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a standard solution containing 0.01500 M Ca2+ required 42.87 mL of EDTA to reach the endpoint. The molarity of the EDTA solution is: ________ M b) That same EDTA solution was then used to titrate an unknown hard water sample. A 40.00 mL aliquot of unknown hard water required 34.21 mL of EDTA solution to reach a distinct endpoint. The concentration of Ca2+ ions (assuming...
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5...
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5Fe3+ (aq) + Mn2(aq) + 4H2O(1) In part A of the experiment, suppose that 1.067 g of Fe(NH4)2(SO4)2.6H2O(s) are placed in a 250 ml Erlenmeyer flask to which 20 mL of water and 8 mL of 3 M H2SO4(aq) are added. The solution was titrated to the end point by adding 26.89 mL of KMnO4(aq) from the...
A sample of an unknown containing Fe2+ in the dissolved sample requires 23.15 mL of a...
A sample of an unknown containing Fe2+ in the dissolved sample requires 23.15 mL of a 0.0020 M KMnO4 solution to reach the end point of the titration. 1)Calculate the moles of KMnO4 reacted. 2) Based on the moles you calculated , calculate how many grams of Fe2+ are in the unknown solution.
7.83 ml of a solution of Fe2+(aq) is titrated with 24.9 ml of 0.375 M KMnO4...
7.83 ml of a solution of Fe2+(aq) is titrated with 24.9 ml of 0.375 M KMnO4 in acidic solution. The balanced Redox equation is: MnO4 (aq) + 5 Fe2+(aq) + 8 H+(aq) --> 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(1) Calculate the concentration, in M, of Fe2+(aq) in the sample. Express your answer to the appropriate number of significant figures.
The Fe2+ (55.845 g/mol) content of a 2.370 g steel sample dissolved in 50.00 mL was...
The Fe2+ (55.845 g/mol) content of a 2.370 g steel sample dissolved in 50.00 mL was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 39.51 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per grams of steel (g Fe2+1 g steel). Mno, +8H+ + 5Fe2+ = Mn2+ + 5Fe'+ + 4H,0 Number g Fe2+1 g steel
suppose you have an unknown sample containing Fe^2+, and you
titrate it with KMnO4 standard solution. Calculate the percent of
Fe in your sample.
equation: MnO4- + 5Fe^2+ + 8H^+ --> Mn^2+ + 5Fe^3+ +
4H2O
Suppose you have an unknown sample containing Feat, and you titrate it with a KMnO4 standard solution. Calculate the percentage of Fe in your sample. Equation: MnO(+5Fe2+ + 8H - Mn2+ + 5Fe3+ + 4H20 Data 0.08124M 2.49g Molarity of the KMnO4 standard solution:...
The Fe2+ (55.845 g/mol) content of a 2.264 g steel sample dissolved in 50.00 mL of an acidic solution was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 44.82 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per gram of steel Mn2+5 Fe34 H20 + 5 Fe2+ MnO8 H concentration g Fe/g steel A 1.969 g...
• CIU TEXAS INSTRUM 2. A 50.00 ml sample of solution containing Fe?ions is titrated with a 0.0216 M KMnO4 solution. It required 20.62 ml of the KMnO4 solution to oxidize all the Fe? ions to Fe ions by the reaction: MnO4 (aq) + Fe? ) -------> Mn(ed) Felco (unbalanced) a) What was the concentration of Fel.ions in the sample solution? b) What volume of 0.0150 M K2Cr2O7 solution would it take to do the same titration? The reaction is:...
The iron content of iron ore can be determined by titration with a standard KMnO4 solution. The iron ore is dissolved in HCl, and all the iron is reduced to Fe2+ ions. This solution is then titrated with KMnO4 solution, producing Fe3+ and Mn2+ ions in acidic solution. If it required 29.83 mL of 0.0447 M KMnO4 to titrate a solution made from 1.128 g of iron ore, what is the mass percent of iron in the iron ore? Mass...
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5Fe3+ (aq) + Mn2(aq) + 4H2O(1) In part A of the experiment, suppose that 1.067 g of Fe(NH4)2(SO4)2.6H2O(s) are placed in a 250 ml Erlenmeyer flask to which 20 mL of water and 8 mL of 3 M H2SO4(aq) are added. The solution was titrated to the end point by adding 26.89 mL of KMnO4(aq) from the...
7.83 ml of a solution of Fe2+(aq) is titrated with 24.9 ml of 0.375 M KMnO4 in acidic solution. The balanced Redox equation is: MnO4 (aq) + 5 Fe2+(aq) + 8 H+(aq) --> 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(1) Calculate the concentration, in M, of Fe2+(aq) in the sample. Express your answer to the appropriate number of significant figures.
The Fe2+ (55.845 g/mol) content of a 2.370 g steel sample dissolved in 50.00 mL was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 39.51 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per grams of steel (g Fe2+1 g steel). Mno, +8H+ + 5Fe2+ = Mn2+ + 5Fe'+ + 4H,0 Number g Fe2+1 g steel
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