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23. The iron present in a sample of iron ore is converted to Fe2+ and titrated...
A sample of iron ore weighing 0.6428g is dissolved in acid, the iron is reduced to...
A sample of iron ore weighing 0.6428g is dissolved in acid, the iron is reduced to Fe2+, and the solution is titrated with 36.30 mL of 0.01753 M K2Cr2O7 solution. The reaction is 6Fe2+ + Cr2O72- +14H+ à 6Fe3+ + 2Cr3+ + 7H2O What is the Percentage of iron (55.85g/mol) in the sample?
A 250.0 mL sample of spring water was treated to convert any iron present to Fe2+...
A 250.0 mL sample of spring water was treated to convert any iron present to Fe2+ . Addition of 24.00 mL of 0.002543 M K2Cr2O7 resulted in the reaction 6Fe2+ + Cr2O7 2- + 14H+ 6Fe3+ + 2Cr3+ + 7H2O The excess K2Cr2O7 was back titrated with 8.02 mL of 0.00971 M Fe2+ solution. Calculate the concentration of iron in the sample in ppm. Please be specific and include details.
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...
The reaction between iron(II) ( Fe2+ ) and dichromate ( Cr2O2−7 ) in the presence of...
The reaction between iron(II) ( Fe2+ ) and dichromate ( Cr2O2−7 ) in the presence of a strong acid ( H+ ) is shown. Cr2O2−7+6Fe2++14H+⟶2Cr3++6Fe3++7H2O Determine the volume, in milliliters, of a 0.180 M solution of Mohr's salt ( (NH4)2Fe(SO4)2⋅6H2O ) needed to completely react with 0.0500 L of 0.180 M potassium dichromate ( K2Cr2O7 ). volume? ... mL What volume, in milliliters, of 0.180 M K2Cr2O7 is required to completely react with 0.0500 L of a 0.180 M solution...
6) A chemist tested the concentration of a stock solution of iron (11) using dichromate solution...
6) A chemist tested the concentration of a stock solution of iron (11) using dichromate solution as a titrant. The reaction between the titrant and the analyte is as follows: 6Fe2+ (aq) + Cr2072 (aq) + 14H+ (aq) → 2Cr3+ + 6Fe3+ + 7H20 A 50.0mL sample of the stock solution required 33.3mL of 2.50x10-2M dichromate titrant to reach the endpoint. What was the concentration of the stock solution?
An iron ore sample weighing 0.5562 g is dissolved HCl (aq), and the iron is obtained...
An iron ore sample weighing 0.5562 g is dissolved HCl (aq), and the iron is obtained as Fe2+ in solution. This solution is then titrated with 28.72 mL of 0.04021 M K2Cr2O7 (aq). What is the percent by mass iron in the ore sample? How do I get to the equation 6Fe^2+ + 14H^+ + Cr2O7^2- ----> 6Fe^3+ + 2Cr^3+ + 7H2O ??? I am just generally confused on how to start this and how to do this step by...
A 0.1362g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as...
A
0.1362g iron ore sample was dissolved in hydrochloric acid and the
iron was obtained as Fe^2+(aq). The iron solution was titrated with
Ce4+ solution according to the balanced chemical reaction shown
below. After calculation, it was found that 0.0238g of iron from
the ore reacted with the cerium solution.
Ce^4+(aq) + Fe 2+(aq) -> Ce^3+(aq) + Fe^3+(aq).
Calculate the mass percent of iron in the original ore sample.
Please round your answer to the tenths place.
Question 7 (2...
The amount of iron in steel can be determined by titration with dichromate. First, the steel...
The amount of iron in steel can be determined by titration with dichromate. First, the steel is dissolved in hydrochloric acid to oxidize all the iron to Feat. An indicator is added that will react with excess dichromate. Then, potassium dichromate is added to the solution until the end point is reached. Cr, 02- +6Fe2+ + 14H+ > 2Cr3+ +6Fe3+ + 74,0 For the analysis of 2.00 g of steel, the titration required 22.70 mL of 0.1800 M K2Cr207. What...
An unknown concentration of HCl is titrated using known KOH. What is the molarity of an...
An unknown concentration of HCl is titrated using known KOH. What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are titrate a 25.0 mL sample of the acid? Final answer: 0.218 M HCI questions, each has 10 points. An unknown concentration of HCl is titrated using known KOH.
A solution of iron (II) sulfate was prepared by dissolving 10.00g of FeSO4-7H20 (FW= 277.9) in...
A solution of iron (II) sulfate was prepared by dissolving 10.00g of FeSO4-7H20 (FW= 277.9) in water and diluting up to a total volume of 250 ml. The solution was left to stand, exposed to air, and some of the iron (II) ions became oxidized to Iron (III) ions. a 25.0 ml sample of this partially oxidized solution required 23.70 ml of 0.0100M potassium dichromate K2Cr2O7 solution for complete reaction in the presence of dilute sulfuric acid. Calculate the percentage...
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...
6) A chemist tested the concentration of a stock solution of iron (11) using dichromate solution as a titrant. The reaction between the titrant and the analyte is as follows: 6Fe2+ (aq) + Cr2072 (aq) + 14H+ (aq) → 2Cr3+ + 6Fe3+ + 7H20 A 50.0mL sample of the stock solution required 33.3mL of 2.50x10-2M dichromate titrant to reach the endpoint. What was the concentration of the stock solution?
A
0.1362g iron ore sample was dissolved in hydrochloric acid and the
iron was obtained as Fe^2+(aq). The iron solution was titrated with
Ce4+ solution according to the balanced chemical reaction shown
below. After calculation, it was found that 0.0238g of iron from
the ore reacted with the cerium solution.
Ce^4+(aq) + Fe 2+(aq) -> Ce^3+(aq) + Fe^3+(aq).
Calculate the mass percent of iron in the original ore sample.
Please round your answer to the tenths place.
Question 7 (2...
The amount of iron in steel can be determined by titration with dichromate. First, the steel is dissolved in hydrochloric acid to oxidize all the iron to Feat. An indicator is added that will react with excess dichromate. Then, potassium dichromate is added to the solution until the end point is reached. Cr, 02- +6Fe2+ + 14H+ > 2Cr3+ +6Fe3+ + 74,0 For the analysis of 2.00 g of steel, the titration required 22.70 mL of 0.1800 M K2Cr207. What...
An unknown concentration of HCl is titrated using known KOH. What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are titrate a 25.0 mL sample of the acid? Final answer: 0.218 M HCI questions, each has 10 points. An unknown concentration of HCl is titrated using known KOH.
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