Final answer in 3 significant figures Chrome then curiously asked Senku if it was possible to titrate the pure KHA.H2A2H20 sample through other titrimetric methods besides the use of acidsand bases. After explaining the concept of redox titrations, Senku thenchallenged you to hypothetically determine the following if the ion A in thecompound was C202² and a KMNO4 solution was used as the titrant.d) How many moles of KMNO4 would react with the KHC2O4 . H2C2O4 2H20sample in acidic media? Show the balanced chemical reaction as well.e) Determine the Gibbs energy change per mole of reaction. Faraday'sconstant is 96485C/mol and the standardreduction potentialsare Emno4-IM12+ =1.507 VECO2H2C204= -0.432 V. Indicate whether it is spontaneous orandnonspontaneous.

Answered: Image /qna-images/answer/4d591e6f-7a7b-4ce5-b50b-c572dc798242.jpg

Chrome then curiously asked Senku if it was possible to titrate the pure KHA. H2A2H;O sample through other titrimetric methods besides the use of acids and bases. After explaining the concept of redox titrations, Senku then challenged you to hypothetically determine the following if the ion A in the compound was C20,² and a KMNO4 solution was used as the titrant. d) How many moles of KMNO4 would react with the KHC2O4 . H2C2O4 2H2O sample in acidic media? Show the balanced chemical reaction as well. e) Determine the Gibbs energy change per mole of reaction. Faraday's constant is 96485 C/mol and the standard reduction potentials are Emno4- Mn2+ =1.507 V and ECO2H2C204= -0.432 V. Indicate whether it is spontaneous or nonspontaneous.

Chrome then curiously asked Senku if it was possible to titrate the pure KHA. H2A2H;O sample through other titrimetric methods besides the use of acids and bases. After explaining the concept of redox titrations, Senku then challenged you to hypothetically determine the following if the ion A in the compound was C20,² and a KMNO4 solution was used as the titrant. d) How many moles of KMNO4 would react with the KHC2O4 . H2C2O4 2H2O sample in acidic media? Show the balanced chemical reaction as well. e) Determine the Gibbs energy change per mole of reaction. Faraday's constant is 96485 C/mol and the standard reduction potentials are Emno4- Mn2+ =1.507 V and ECO2H2C204= -0.432 V. Indicate whether it is spontaneous or nonspontaneous.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.34QAP

See similar textbooks

Similar questions

Using basic conditions, MnO4- can be used as titrant for the analysis of Mn2+, with both the analyte and the titrant ending up as MnO2. In the analysis of a mineral sample for manganese, a 0.5165-g sample is dissolved, and the manganese is reduced to Mn2+. The solution is made basic and titrated with 0.03358 M KMnO4, requiring 34.88 mL to reach the endpoint. Calculate the %w/w Mn in the mineral sample. Answer: % Mn =
The level of dissolved oxygen in a water sample can be determined by the Winkler method. In a typical analysis, a 100.0-mL sample is made basic, and treated with a solution of MnSO4, resulting in the formation of MnO2. An excess of KI is added, and the solution is acidified, resulting in the formation of Mn2+ and I2. The liberated I2 is titrated with a solution of 0.00870 M Na2S2O3, requiring 8.90 mL to reach the starch indicator end point. Calculate the concentration of dissolved oxygen as parts per million of O2.
In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. Accordingly, what is the concentration of KMnO4?
An analysis for borohydride ion is based on its reaction with Ag+: BH4- + 8Ag+ + 8OH--> H2BO3- + 8Ag(s) + 5H2O The purity of a quantity of KBH4 to be used was established by diluting 3.213 g of the material to exactly 500.0 mL, treating a 100.0-mL aliquot with 50.00 mL of 0.2221 M AgNO3, and titrating the excess silver ion with 3.36 mL of 0.0397 M KSCN. Calculate the percent purity of the KBH4 (53.941 g/mol).
The protein content of wheat flour can be determined reasonably accurately by multiplying the percentage of nitrogen present by 5.7. A 2.06-g sample of flour was taken through a Kjeldahl procedure and the ammonia produced was distilled into a boric acid solution. If this solution required 34.70 mL of 0.174 N HCl for titration to the methyl red end point, what is the a) % Nitrogen and b) % protein in the flour? (Use 1:1 stoich ratio between N and HCl)
Give only typing answer with explanation and conclusion 0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol)
If Sn3(PO4)2 solution is to be subjected to argentometric titration, a) Write the balanced titration reaction. (products are Ag3PO4(s),, other ions are spectator ions b) Write the stoichiometric relationship (fundamental eqn) between the titrant (AgNO3) and the titrand (Sn3(PO4)2. c) Is this a feasible titration technique? Why?
In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. What is the KMnO4 concentration?
The amount of sulfate in a solid sample was determined by first dissolving 562.2 mg of sample in water, and then precipitating the sulfate by the addition of 25.00 mL of 0.022 96 M BaCl2. The precipitate was filtered from the solution and the remaining Ba2+ was titrated with 16.52 mL of 0.014 57 M EDTA. What was the mass percent of sulfate in the solid?
While working in a metal processing facility, Letlen had accidentally mixed two metal vatstogether creating an alloy. One vat was labeled for cadmium, while the other was not. It canbe assumed that these are of pure metal composition. To identify this metal, Letlen took 1.000 g of the homogenous alloy sample composed ofcadmium and the unknown metal, dissolved, and diluted it to exactly 100.0 mL in avolumetric flask. A 20.00-mL aliquot was taken and titrated this using 22.82 mL of 0.05000M EDTA. In a second 20.00-mL aliquot, the Cd was masked through the addition of HCN/NaCN buffer.The titration of the unknown metal in the aliquot required 15.13 mL of EDTA.MW: Cd (112.411 g/mol) a. Calculate the moles of Cd and the moles of unknown metal in the 20.00-mL aliquot.b. Calculate the moles of Cd and the moles of unknown metal in the sample.
An acidic solution of copper (.35 M Cu+2) was treated with KOH until Cu(OH)2 precipitated. At what pH does this occur at?
A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca C) The percentage of CaO