1)
No. of moles of MnO4- required = molarity x volume
= 0.0244 x 36.44
= 0.889 millimoles
change in oxidation state = 5
change in oxidation state = 1
Thus no. of moles of Fe present = 5 / 1 x 0.889
= 4.45 millimoles
Mass of iron present = 4.45 / 1000 x 56 g / mol
= 0.249 g
1. A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M...
PRE-LAB ASSIGNMENT 1) Write the balanced net ionic equation for the reaction between MnO4-ion and Feation in acid solution. 2) How many moles of Fe²+ ion can be oxidized by 1.2 X 10-2 moles of MnO4 in the above reaction? moles 3) A solid sample containing some Fetion weighs 1.750 g. It requires 36.44 ml of 0.0244 M KMnO4 to titrate the Fe in the dissolve sample to pink end point. a. How many moles of MnO4- are required? moles...
An acidified solution of manganate (VII) of permanganate ions, MnO4-, is a strong oxidising agent and will be used in an experiment to determine the percentage of iron in a sample of ammonium iron (II) sulfate hexahydrate. The titration is self-indicating because at the equivalence point the products are a different colour than the original reactants. The two half reactions are: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l) Fe^2+(aq) ---> Fe^3+(aq) + e- a) What is a redox...
You wish to prepare 250.0250.0 mL of a 225.0225.0 ppm w/v Fe2+Fe2+ (MW=55.845 g/molMW=55.845 g/mol) solution. How many grams of ferrous ammonium sulfate hexahydrate (Fe(NH4)2(SO4)2⋅6H2O(Fe(NH4)2(SO4)2⋅6H2O, MW=392.14 g/molMW=392.14 g/mol) are needed to prepare this solution? Assume the final solution has a density of 1.00 g/mL.
Spring 2019 CSUSM CHEM 175 8. Which statements are true? Select ALL. that apply. a) Dissolution of ammonium nitrate is an endothermic reactio b) Hydrogen gas evolves when calcium carbonate reacts with hydrochloric acid. c) The acid-base neutralization reaction is exothermic. ) The value of enthalpy change, AH, of calcium chloride dissolution is positive. sample contains an unknown amount of Fe?'which is titrated with a KMnO, solution in acidie tions to determine the iron composition by mass. A standardized KMnOs...
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.
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:...
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...
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+ (55.845 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...