Homework Answers
a) Here
Volume of Fe2+ solution = 50ml
Volume of kMnO4- solution = 20.62ml
Molarity of kMnO4-solution = 0.0216M
Balanced Reaction
No. of moles of KMnO4 = Molarity x Volume
= 0.0216 x 20.62
= 0.445392 mol.
According to reaction
b) Here, Concentration of K2Cr2O7 = 0.0150 M
Add Answer to:
• CIU TEXAS INSTRUM 2. A 50.00 ml sample of solution containing Fe?ions is titrated with a 0.0216 M KMnO4 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.
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:...
4. A 0.5255 g sample containing an unknown mass of SnCl2 is dissolved in 50.00 mL...
4. A 0.5255 g sample containing an unknown mass of SnCl2 is dissolved in 50.00 mL of water and titrated with 0.02050 M KMnO4 under mildly acidic conditions. The unbalanced titration reaction is shown below. MnO4 (aq) + Sn²(aq) MnO2(8) + Sn** (aq) a. Use the half-reaction method to balance the titration reaction. (5 pts) b. Given that 32.25 mL of KMnO, was required to reach the endpoint, calculate the percent SnCl2 in the sample. (5 pts)
7.41 ml of a solution of Fe2+ (aq) is titrated with 19.3 ml of 0.367 M...
7.41 ml of a solution of Fe2+ (aq) is titrated with 19.3 ml of 0.367 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.
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...
4. A 2.86 g sample containing both Fe and V was dissolved under certain conditions and diluted to 200.00 mL. Fe2 and VO ions. The titration of this solution required 22.64 mL of0.1000 M Ce" t...
4. A 2.86 g sample containing both Fe and V was dissolved under certain conditions and diluted to 200.00 mL. Fe2 and VO ions. The titration of this solution required 22.64 mL of0.1000 M Ce" to reach end point. A second 50.00 mL aliquot was passed through a Jones reductor to forn ions. The titration of the second solution required 42.66 mL of 0.1000 M Ce solution to reach an end point. Calculate the percentage of Fe and V in...
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...
? Fe (ag) reacts with MnO Caq) ion in acidic solution to yield Fe (ag) ions...
? Fe (ag) reacts with MnO Caq) ion in acidic solution to yield Fe (ag) ions and Mn'(a) ions. 5 Fe"(aq) + Mno.(aq) + 8H' ? 5 Fe"(aq) + Mn"(aq) + 4H20 A sample of melanterite, FeSO, 7H,O, was analyzed for purity using this reaction by titration of an aqueous solution of the sample. One such sample required 56.15 mL of 0.01301 M permanganate solution to completely titrate all the iron in the sample by the reaction shown above. How...
A 1.026 g sample of an iron unknown requires 24.35 mL of 0.0195 M MOA solution...
A 1.026 g sample of an iron unknown requires 24.35 mL of 0.0195 M MOA solution to reach the end point. The atomic mass of Fe is 55.85 g/mol. Balanced equation: 5Fe2+ (aq) + MnO4 (aq) + 8H(aq) 5Fe(aq) + Mn(aq) + 4H2O) Which species aids in the dissolution of the compounds and helps to facilitate the reaction? Spectator ions are omitted. c) H b) Fe3+ d) Mn2+ a) MnO4 What is the mass percent of iron in the unknown?...
18. A 25.00 ml sample of the 50.00 ml solution was titrated with 0.1359 M potassium...
18. A 25.00 ml sample of the 50.00 ml solution was titrated with 0.1359 M potassium thiocyanate and 12.90 mL were required to reach the endpoint. Calculate the gram of silver (MM= 107.87 g/mol) in the sample.
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.
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:...
4. A 0.5255 g sample containing an unknown mass of SnCl2 is dissolved in 50.00 mL of water and titrated with 0.02050 M KMnO4 under mildly acidic conditions. The unbalanced titration reaction is shown below. MnO4 (aq) + Sn²(aq) MnO2(8) + Sn** (aq) a. Use the half-reaction method to balance the titration reaction. (5 pts) b. Given that 32.25 mL of KMnO, was required to reach the endpoint, calculate the percent SnCl2 in the sample. (5 pts)
7.41 ml of a solution of Fe2+ (aq) is titrated with 19.3 ml of 0.367 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.
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...
4. A 2.86 g sample containing both Fe and V was dissolved under certain conditions and diluted to 200.00 mL. Fe2 and VO ions. The titration of this solution required 22.64 mL of0.1000 M Ce" to reach end point. A second 50.00 mL aliquot was passed through a Jones reductor to forn ions. The titration of the second solution required 42.66 mL of 0.1000 M Ce solution to reach an end point. Calculate the percentage of Fe and V in...
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...
? Fe (ag) reacts with MnO Caq) ion in acidic solution to yield Fe (ag) ions and Mn'(a) ions. 5 Fe"(aq) + Mno.(aq) + 8H' ? 5 Fe"(aq) + Mn"(aq) + 4H20 A sample of melanterite, FeSO, 7H,O, was analyzed for purity using this reaction by titration of an aqueous solution of the sample. One such sample required 56.15 mL of 0.01301 M permanganate solution to completely titrate all the iron in the sample by the reaction shown above. How...
A 1.026 g sample of an iron unknown requires 24.35 mL of 0.0195 M MOA solution to reach the end point. The atomic mass of Fe is 55.85 g/mol. Balanced equation: 5Fe2+ (aq) + MnO4 (aq) + 8H(aq) 5Fe(aq) + Mn(aq) + 4H2O) Which species aids in the dissolution of the compounds and helps to facilitate the reaction? Spectator ions are omitted. c) H b) Fe3+ d) Mn2+ a) MnO4 What is the mass percent of iron in the unknown?...
18. A 25.00 ml sample of the 50.00 ml solution was titrated with 0.1359 M potassium thiocyanate and 12.90 mL were required to reach the endpoint. Calculate the gram of silver (MM= 107.87 g/mol) in the sample.
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