2) Under acidic conditions, an aqueous solution of permanganate ion is often used to oxidize an aqueous solution of Iron II to an aqueous solution of Iron III ion. In addition, the permanganate ion is reduced to an aqueous solution of the Manganese II ion. A 50.00 mL sample of solution containing the Iron II ions is titrated with 20.62 mL of a 0.0216 M potassium permanganate solution to oxidize all the Iron II ions. What was the concentration of Iron II ions in the original 50.00 mL sample?

2) Under acidic conditions, an aqueous solution of permanganate ion is often used to oxidize an aqueous solution of Iron II to an aqueous solution of Iron III ion. In addition, the permanganate ion is reduced to an aqueous solution of the Manganese II ion. A 50.00 mL sample of solution containing the Iron II ions is titrated with 20.62 mL of a 0.0216 M potassium permanganate solution to oxidize all the Iron II ions. What was the concentration of Iron II ions in the original 50.00 mL sample?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Write the balanced net ionic equation for the precipitation of lead (II) hydroxide from aqueous solution: write the balanced net ionic equation for the precipitation of chromium (iii) sulfide from aquesous solution:
The molarity of sulfuric acid in a fully charged car battery is 5.2 M. When fully discharged the molarity is 4.8 M. A 2.00 mL sample of battery acid was titrated with 31.26 mL if a 0.621 M sodium hydroxide solution. Does the battery need to be recharged? Document your answer.
A sample of battery acid is to be analyzed for its sulfuric acid content. A 1.00-mL sample weighs 1.256 g . This 1.00-mL sample is diluted to 250.0 mL, and 10.00 mL of this diluted acid requires 34.89 mL of 4.522×10−3 M Ba(OH)2 for its titration. What is the mass percent of H2SO4 in the battery acid? Enter a numerical answer only, in terms of percent but do not include the "%".
8b and 16c
An aqueous solution of hydrobromic acid is standardized by titration with a 0.120 M solution of barium hydroxide.If 11.7 mL of base are required to neutralize 22.1 mL of the acid, what is the molarity of the hydrobromic acid solution?M hydrobromic acid
All the chloride in a 5.00 g sample of an unknown metal chloride is precipitated as AgCl with 70.9 mL of 0.2010 M AgNO3. What is the percentage of chloride in the sample?
6. The following reaction forms a white precipitate. Is this a redox reaction? AgNO3(aq) + HCl(aq) → HNO3(aq) + AgCl(s)
A sample of iron ore is dissolved in acid, and the iron is converted to Fe2+ (iron II). The sample is then titrated with 57.30 mL of 0.03240 M MnO4- solution. The net ionic equation for the oxidation-reduction that occurs during titration is as follows: Mn04-(aq) + 5FE2+(aq) + 8H+(aq) --> Mn2+(aq) + 5FE3+(aq) + 4H2O(I) How many moles of Fe2+ were in the sample? O 2.269 x 10^-2 mol (2.269E-2 mol) O 7.563 x 10^-3 mol (7.563E-3 mol) O 9295.1 mol O 5 mol O 9.285 x 10^-3 mol (9.285E-3 mol)
Does a reaction occur when aqueous solutions of sodium carbonate and manganese(II) iodide are combined? O yes no If a reaction does occur, write the net ionic equation. (Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank.) + →
One method of determining the concentration of hydrogen peroxide (H₂O₂) in a solution is through titration with iodide ion. The unbalanced net ionic equation for this reaction is H₂O₂ +1+H* → 1₂ + H₂O A 50.00 mL sample of a hydrogen peroxide solution is found to react completely with 37.12 mL of a 0.1500 M KI solution. What is the concentration of hydrogen peroxide in the sample? O a. 0.2227 M O b. 0.4041 M O c. 0.1010 M O d. 5.568 x 10-² M 17.5 mL of a 0.1050 M Na₂CO3 solution is added to 46.0 mL of 0.1250 M NaCl. What is the concentration of sodium ion in the final solution? O a. 0.119 M O b. 0.148 M O c. 0.539 M O d. 0.205 M
11. What volume of a 0.2087 M solution of permanganate ion (under basic conditions) will react with 27.00 mL of .0990 M sulfite ion solution. Manganese(II) oxide solid and sulfate ions are the products. If0 2500 g sample of an unknown triprotic acid is neutralized by 14.2 mL of 0.187 M stron
A 25.00 mL aliquot is withdrawn from the liquid portion of saturated Manganese (II) hydroxide and transferred to an Erlenmeyer flask. After the addition of methyl orange, a titration with 0.0045 M HCl was performed. The endpoint was reached after 8.72 mL of the acid was added. What is the balanced chemical equation? How many moles of hydroxide ions were neutralized in the reaction? What is the molar concentration of hydroxide in the saturated solution? What is the molar concentration of Magnesium ion in solution?