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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...
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 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
The Fe2+ (55.84555.845 g/mol) content of a 2.028g steel sample dissolved in 50.00mL of an acidic solution was determined...
The Fe2+ (55.84555.845 g/mol) content of a 2.028g steel sample dissolved in 50.00mL of an acidic solution was determined by tiration with a standardized 0.130 M potassium permanganate (KMnO4KMnO4, 158.034 g/mol) solution. The titration required 36.61 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. MnO−4+8H++5Fe2+↽−−⇀Mn2++5Fe3++ concentration: ______________ g Fe/g steel
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 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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Learning Outcomes:
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> It says that the sample was dissolved and an aliquot was added, therefore we need to compute for the mass of the sample per aliquot, also the stoichiometry doesn't work that way in James and Walden Reductors. Try computing for the mole of Ce4+ then relating it to the moles of vanadium + moles of iron per type of reductor
Zack Fair Sun, Mar 27, 2022 11:05 PM