The amount of Fe in a 0.4891-g sample of an ore is determined by titrating with K2Cr207. After dissolving the sample in HCI, the iron is brought into a +2 oxidation state using a Jones reductor. Titration to the diphenylamine sulfonic acid end point requires 36.92 mL of 0.02153 M K2Cr207. Report the ore's iron content as %w/w Fe203. In this problem, which is the titrant? O K2Cr207 O diphenylamine sulfonic acid Fe203 HCI Fe2+

The amount of Fe in a 0.4891-g sample of an ore is determined by titrating with K2Cr207. After dissolving the sample in HCI, the iron is brought into a +2 oxidation state using a Jones reductor. Titration to the diphenylamine sulfonic acid end point requires 36.92 mL of 0.02153 M K2Cr207. Report the ore's iron content as %w/w Fe203. In this problem, which is the titrant? O K2Cr207 O diphenylamine sulfonic acid Fe203 HCI Fe2+

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

Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL The solution was diluted in H20, Fe(lII) was precipitated as Fe2O3.H20 by adding NH3. After filteration, washing the residue ignited to give 0.2697 g of pure Fe2Os (159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample. O 16.66 % O 69.12 % O 54.21 % 45.21 % 33.32 % hp
Balance the equation in basic conditions. Phases are optional. equation: CoCl, + Na,O, Co(OH), + Cl + Na+ >
3. Calculate the [Ag"] in a solution prepared by dissolving 1.00 g of AgNO3 and 10.0g KCN in enough water to make 1.00 L of solution. Kf[Ag(CN)2] = 1.0 x 102 1-
Explain why copper(II) and iodide ions do not co-exist in acidic solution but do co-exist in the presence of ammonia. I want solution ASAP
1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution. Box the final answer.
Find the pH value for a solution containing 0.5 mg/L of copper ion (Cu2+) dissociated from Cu(OH)2 at equilibrium. If the pH of this solution is adjusted to 6 and 10, what would be the concentrations of copper ion in mg/L at equilibrium, respectively?
What is the oxidation state of Fe in the molecule Fe203?
This method requires acidic conditions to prevent iron from precipitating out as ferric hydroxide EDTA Fajans Volhard Mohr
A solution is prepared by mixing the two solutions together. The first solution is 150.0 mL and contains 30.78 mM Ti3+, 29.40 mM Ce3+, and 8.75 mM HCI. The second solution is 200.0 mL and contains 40.23 mM EDTA and 11.48 mM piperidine. Determine the concentration of free (non-complexed) metals when the two solutions are mixed.
A mined alloy sample weighing 2.0840 g is dissolved in minimal amounts of concentrated HNO3 before diluted to 50 mL. Ten mL of this diluted sample was titrated using 0.091 M KSCN and required 14.20 mL to reach the endpoint. Calculate the concentration of silver (%w/w) in the mined alloy. (Hint: A dilution factor (DF) is needed in the formula.) Titration reaction: Agt + SCN- → A9SC'N(s) FW: Ag = 107.87 %3D
Write a balanced net ionic equation to show why the solubility of Cu(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Be sure to specify states such as (aq) or (s). + + K =
A sample of an iron ore was prepared for Fe3+ analysis as following: 3.4g of the sample was added anddissolved in acid environment then diluted to 250 mL using volumetric flask. After that, 10 mL of the resultingsolution was transferred by pipet to a 50-mL volumetric flask and continue to be diluted. The scientists foundout that this solution gives the concentration of Fe3+ as 2.3 mg/L. Find the weight percentage of Fe3+ in theoriginal sample.