2) A 100.0-mL sample of spring water was treated to convert any iron present to Fe2*.Addition of 25.00 mb. of 0.008 M K2Cr207 resulted in the reaction6F22+ + Cr2O72- + 14H*2 6FE3+ + 2Cr3+ + 14H2OThe excess K2C12O7 was back-titrated with 8.53 ml of 0.00949 M Fe2* şolution. Calculate themolar concentration of iron in the sample.

Answered: The excess K2Cr207 was back-titrated…

The excess K2Cr207 was back-titrated with 8.53 ml of 0.00949 M Fe2* şolution. Calculate the molar concentration of iron in the 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

Related questions

Q: 0.7120 g of iron ore was dissolved and the iron was reduced to Fe2+ with Jones's reagent. Fe(II) was…

A: Here we are required to find the % Of Fe and Fe2O3 in the 0.712 g of iron Ore. The iron present in…

Q: A 0.8040-g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe21 and titrated…

A: Initially from the given balanced equation Mole ratio is found and then moles of Fe and Fe2O3 are…

Q: 5.3 A 0.1200 g sample of pure iron wire was dissolved in acid, reduced to +2 state and titrated with…

A: 5.3 A 0.1200 g sample of pure iron wire was dissolved in acid and reduced to +2 oxidation state .…

Q: In Questions 1 through 6, you will be calculating the initial concentrations of Fe³+ ([Fe³+]o) and…

A: #QUESTION 1: Each Fe(NO3)3(aq) is completely dissociated into 1 Fe3+(aq). Hence [Fe(NO3)3(aq)] =…

Q: A 110.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of…

A: Answer is 172.4 ppm

Q: A mixture of solid chlorides was known to contain some or all of the following cations: Ag…

A: Out of the given possibility of chlorides of Ag+, Al3+, Cr3+, Ca2+ and Zn2+, only AgCl is not…

Q: 93 Chemistry I Laboratory Manual, 2019 Revision Questions: gy muibor alo vialom od W (E 1) Samples…

A: a. The species that is oxidised is Fe2+ b. The species that is reduced is Cr2O7^2-

Q: A 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric…

A: Answer: This question is based on stoichiometric calculation where moles of SCN- needs to be…

Q: Use the solubility product to determine whether CaHPO4 will precipitate from a solution with [Ca2+]…

A: Given, Concentration of Ca2+ = 0.0001M. Concentration of HPO42- = 0.001M.

Q: Provide the balanced net ionic chemical equation for the oxidation-reduction reaction between Fe 2+…

A: Given Fe2+ It will under go oxidation Fe2+ ← Fe3+2. Cr2 O7 2- Oxidation state of Cr = +6undergo…

Q: Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation :…

A: Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation :…

Q: An impure sample H2C2O4 was oxidized by KMnO4. A 0.262g sample of H2C2O4 was dissolved, and the…

A: The question is based on the concept of titrations. we are titrating oxalic acid with potassium…

Q: TI Pt Cr3+ (1 M) Cr2+ (1 M) T13+ (1 M) T13+ (aq) + 3e- TI (s) Cr2+ (aq) → Cr3+ (aq) + e- The species…

Q: A sample of copper oxide weighing 2.013 g is dissolved in acid, the pH adjusted, and excess KI…

Q: The iron content of a mineral deposit was determined by titration with KMNO4 to see if it had enough…

Q: A o.8024 g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe2" and titrated…

Q: To analyze the amount of iron (Fe; Mw = 55.85 g/mol) contained in an ore sample, the sample was…

A: Given in the question, Volume of EDTA = 25 ml Molarity of EDTA = 0.2922 M Total moles of EDTA =…

Q: Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL, The solution was diluted in…

A: A multiple choice question based on mole concept, which is to be accomplished.

Q: 2. A sample iron ore weighing 0.6428 g is dissolved in acid, the iron is reduce to Fe2*, and the…

Q: The amount of Fe in a 0.4891-g sample of an ore was determined by a redox titration with K2Cr,0,.…

Q: A 0.8040 g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe²+ and titrated…

Q: The hydrogen sulfide in a 40.0-g sample of crude petroleum was removed by distillation and collected…

A: Mass of CdSO4 = 0.079 g Mass of sample = 40.0 g

Question

2) A 100.0-mL sample of spring water was treated to convert any iron present to Fe2*.
Addition of 25.00 mb. of 0.008 M K2Cr207 resulted in the reaction
6F22+ + Cr2O72- + 14H*2 6FE3+ + 2Cr3+ + 14H2O
The excess K2C12O7 was back-titrated with 8.53 ml of 0.00949 M Fe2* şolution. Calculate the
molar concentration of iron in the sample.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What volume of 0.170 M KMnO4 would be required to titrate 0.38 g of K2[Cu(C2O4)2]⋅2H2O?
Balance the following reactions in acidic and basic medium. Al(s) + O2(g) [Al(OH)4] Cr2072- + C2H5OH Cr³* + CO2 H2 + O2 H20 ASH3 + Ag* As406 + Ag
A quantitative analysis for ethanol, C2H60, is accomplished by a redox back titration. Ethanol is oxidized to acetic acid, C2H402, using excess dichromate, 3+ Cr207 2-, which is reduced to Cr3*. The excess dichromate is titrated with Fe2*, giving C and Fe+ as products. In a typical analysis, a 5.00-mL sample of a brandy is diluted to 500 mL in a volumetric flask. A 10.00-mL sample is taken and the ethanol is removed by distillation and collected in 50.00 mL of an 2- acidified solution of 0.0200 M K2Cr207. Titration of the unreacted Cr207 requires 21.48 mL of 0.1014 M Fe2*. Calculate the %w/v ethanol in the brandy. Which is the titrant in this problem? C2H402 Fe2+ C2H60 O Cr207 2-
2. A sample iron ore weighing 0.6428 g is dissolved in acid, the iron is reduce to Fe2+, and the solution is titrated with 36.30 mL of 0.01753 M K,Cr,O, solution. Calculate the percentage of iron (MM=55.85 g/mol) in the sample Rxn: 6 Fe 2* + Cr,072- + 14H* → 2Cr 3* + 6 Fe 3* + 7 H20 analyte titrant
What is the full equation (not the net ionic equation) for the chemical reaction of 0.001 M Fe(NO3)3 plus 0.0002 M NaSCN diluted up to 10 mL with 0.1M HNO3? Please include the acid that is the diluent.
A weighed sample of sodium nitrite was treated with 0.05 mol of ceric sulfate in solution, in air-free conditions. The resulting solution was titrated with standard Fe(II) solution and 0.01 mol of Fe(II) were required. Determine the moles of sodium nitrite present in the weighed sample. NO2– + 2 Ce4+ + H2O → NO3– + 2 Ce3+ + 2 H+ Fe2+ + Ce4+→ Fe3+ + Ce3+
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.
A 20 mL volume of 0.015 M KIO3 containing an excess of KI, is added to a 0.312 g sample of a Real Lemon solution containing vitamin C. The Yellow-brown solution, caused by excess I2 is titrated to a colorless starch endpoint with 11.3 mL pf 0.106M Na2S2O3. Question: Calculate the percent by mass of Vitamin C in the Real Lemon Sample
The hydrogen sulfide in a 75.0-g sample of crude petroleum was removed by distillation and uncollected in a solution of CdCl2. The precipitated CdS was then filtered, washed, and ignited to CdSO4. Calculate the percentage of H₂S in the sample if 0.115 g of CdSO4 was recovered.
You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4 . The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. Determine the dosage strength of the product in terms of % Mg(OH)2 content. Type your answer in 2 decimal places, numbers only.
Write the mass-balance expressions for a solution that is a. 0.38 M in HNO₂. M= b. 0.44 M in (CH3)2NH. M= c. saturated with Ag₂ S. = + + + +
The zinc in a 0.7162-g sample of foot powder was titrated with 21.27 mL of 0.01645 M EDTA. What was the percent zinc in the sample (4 sf)?