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Question 10 (2 points) A 13.9800-g sample of a salt was analyzed for its iron content...
Question 2 (2 points) A 3.2100-g sample of a salt was analyzed for its chloride content...
Question 2 (2 points) A 3.2100-g sample of a salt was analyzed for its chloride content as follows: the entire sample was dissolved with distilled water in a 500.0-ml volumetric flask. A 100.00-mL aliquot of the solution required 24.89-mL of a 0.03769 M silver nitrate solution to reach equivalence. A blank correction was not required. Calculate the % (w/w) chloride in the sample. The net-ionic equation for the reaction is Ag*(aq) + CI (aq) - AgCl(s). Provide your answer to...
I dont know how to do these calculations Volumetric calculations • Example 4: The zinc in...
I dont know how to do these calculations
Volumetric calculations • Example 4: The zinc in a 0.7556-9 sample of foot powder was titrated with 21.27 mL of 0.01654 M EDTA. Calculate the percentage of zinc in the sample. Volumetric calculations • Example 5: A 0.7120-9 specimen of iron ore was brought into solution and passed through a Jones reductor. Titration of the Fe(II) required 39.21 mL of 0.02086 M KMnO4. Express the results of the analysis in terms of...
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...
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
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?...
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
A standard iron solution was prepared by dissolving 0.0100 g of pure iron in acid then...
A standard iron solution was prepared by dissolving 0.0100 g of pure iron in acid then transferring to a 50.00 mL volumetric flask with orthophenanthroline as a complexing agent. At a wavelength of 540 nm, the absorbance of the standard was 0.239 in a 1.00 cm cuvette. A 0.149 g sample of an iron ore was crushed and digested in 5 mL of concentrated acid. The digested sample was then transferred to a 10.00 mL volumetric flask and diluted to...
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:...
(10 pts) The iron content of a well water sample is determined by UV-Vis spectroscopy. A...
(10 pts) The iron content of a well water sample is determined by UV-Vis spectroscopy. A 10.00 mL aliquot of well water is transferred to a 100.0-mL volumetric flask and 20 mL of 0.10 M nitric acid is added to oxidize iron (II) to iron (II). Next 30 mL of a 0.1 M sodium thiocyanate solution is added to form the deep red complex iron (II) thiocyanate. The solution is diluted to volume with DI water. A reagent blank is...
A standard solution of iron was made by weighing 0.075 g of Fe(NH4)2(SO4)2 6(H2O) in 250...
A standard solution of iron was made by weighing 0.075 g of Fe(NH4)2(SO4)2 6(H2O) in 250 mL. Aliquots of this standard solution (see below) were transferred to a 100 mL volumetric flask, pH adjusted with citrate, and reacted with hydroquinone and o-phenanthroline and diluted to volume (100 mL). The absorbance was measured in a 1.0-cm cell using a Genesys 20 Spectrophotometer at 508 nm: Aliquot of standard solution Absorbance 1.0 mL 0.079 2.0 mL 0.163 5.0 mL 0.413 10.0 mL...
Question 2 (2 points) A 3.2100-g sample of a salt was analyzed for its chloride content as follows: the entire sample was dissolved with distilled water in a 500.0-ml volumetric flask. A 100.00-mL aliquot of the solution required 24.89-mL of a 0.03769 M silver nitrate solution to reach equivalence. A blank correction was not required. Calculate the % (w/w) chloride in the sample. The net-ionic equation for the reaction is Ag*(aq) + CI (aq) - AgCl(s). Provide your answer to...
I dont know how to do these calculations
Volumetric calculations • Example 4: The zinc in a 0.7556-9 sample of foot powder was titrated with 21.27 mL of 0.01654 M EDTA. Calculate the percentage of zinc in the sample. Volumetric calculations • Example 5: A 0.7120-9 specimen of iron ore was brought into solution and passed through a Jones reductor. Titration of the Fe(II) required 39.21 mL of 0.02086 M KMnO4. Express the results of the analysis in terms of...
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 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?...
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
A standard iron solution was prepared by dissolving 0.0100 g of pure iron in acid then transferring to a 50.00 mL volumetric flask with orthophenanthroline as a complexing agent. At a wavelength of 540 nm, the absorbance of the standard was 0.239 in a 1.00 cm cuvette. A 0.149 g sample of an iron ore was crushed and digested in 5 mL of concentrated acid. The digested sample was then transferred to a 10.00 mL volumetric flask and diluted to...
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:...
(10 pts) The iron content of a well water sample is determined by UV-Vis spectroscopy. A 10.00 mL aliquot of well water is transferred to a 100.0-mL volumetric flask and 20 mL of 0.10 M nitric acid is added to oxidize iron (II) to iron (II). Next 30 mL of a 0.1 M sodium thiocyanate solution is added to form the deep red complex iron (II) thiocyanate. The solution is diluted to volume with DI water. A reagent blank is...
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