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The reduction potential of Fe2+ is 0.732 volts, and the reduction potential of MnO4 in acidic...
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...
MNO4- reacts with Fe2+ in acidic solution to produce Fe3+. Mn2+. and H2O.
MNO4- reacts with Fe2+ in acidic solution to produce Fe3+. Mn2+. and H2O. Write the balanced half reactions for the oxidation and reduction reactions. Label each reaction as either oxidation or reduction. a) Write the balanced half-reactions for the oxidation and reduction reactions, Label each reaction as either oxidation or reduction. Oxidation reaction: Reduction reaction: b) Write a balanced oxidation-reduction equation for the reaction. TTI Arial 3 (128 : T.E.E.5.
Consider the following UNBALANCED reaction IN ACIDIC SOLUTION: Fe2+(aq) + MnO4-(aq) ⟶ Fe3+(aq) + Mn2+(aq) a....
Consider the following UNBALANCED reaction IN ACIDIC SOLUTION: Fe2+(aq) + MnO4-(aq) ⟶ Fe3+(aq) + Mn2+(aq) a. (5) Species that is oxidized (be specific – i.e. identify which atom and if there are multiple atoms with different charges, identify the correct one) b. (5) Species that is reduced (same instructions as above) c. (10) Full Balanced oxidation ½ reaction (‘full’ means with regard to mass (atoms) and charges.) d. (10) Full Balanced reduction ½ reaction e. (9) Complete Balanced Reaction Using...
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?
EXPERIMENT 7 OXIDATION-REDUCTION TITRATIONS Name HOMEWORK EXERCISES Use the net ionic equations in problems I and...
EXPERIMENT 7 OXIDATION-REDUCTION TITRATIONS Name HOMEWORK EXERCISES Use the net ionic equations in problems I and 2 for problems 3-5 1. a. Write the balanced equations for the half reactions (ionic) and the overall net ionic equation for the titration of Mohr's salt with KMnO4. lonic MnO,: lonic Fe Net ionic: b. What is the standardized molarity of a KMnO4 solution if 36.31 mL are required to titrate 2.5010 g of Mohr's salt? 2. a. Write the balanced equations for...
If the standard reduction potential for A --> A+ + e- was 1.21 volts and the...
If the standard reduction potential for A --> A+ + e- was 1.21 volts and the standard reduction potential for B --> B+2 + 2 e- was 0.46 volts, what would be the standard potential for the following reaction: B+2 + 2 A --> 2 A+ + B? If the standard reduction potential for X --> X+2 + 2 e- was 0.53 volts and the standard potential for the reaction: X + Y+2 --> X+2 + Y was 0.4 volts,...
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:...
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.
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...
E) If the cell potential as measured is 1.04 volts, what would be the reduction potential associa...
Please give the correct answer for (e) the last problem
e) If the cell potential as measured is 1.04 volts, what would be the reduction potential associated with the Ni2+/Ni reaction if the Hg/Flg22+ half-cell is assigned a potential of 0.00 V? Repeat the question: if the Hg/Hg22" half-cell is assigned a reduction potential of -0.80 volts? Hg/Hg2 is 0.00 v: Hg/Hg22* is -0.80 V:
e) If the cell potential as measured is 1.04 volts, what would be the reduction...
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...
EXPERIMENT 7 OXIDATION-REDUCTION TITRATIONS Name HOMEWORK EXERCISES Use the net ionic equations in problems I and 2 for problems 3-5 1. a. Write the balanced equations for the half reactions (ionic) and the overall net ionic equation for the titration of Mohr's salt with KMnO4. lonic MnO,: lonic Fe Net ionic: b. What is the standardized molarity of a KMnO4 solution if 36.31 mL are required to titrate 2.5010 g of Mohr's salt? 2. a. Write the balanced equations for...
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 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...
Please give the correct answer for (e) the last problem
e) If the cell potential as measured is 1.04 volts, what would be the reduction potential associated with the Ni2+/Ni reaction if the Hg/Flg22+ half-cell is assigned a potential of 0.00 V? Repeat the question: if the Hg/Hg22" half-cell is assigned a reduction potential of -0.80 volts? Hg/Hg2 is 0.00 v: Hg/Hg22* is -0.80 V:
e) If the cell potential as measured is 1.04 volts, what would be the reduction...
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