please answer directly with solution no need explanation 2. A 100.0-mL sample of spring water was treated to convert any iron present to Fe2*.Addition of 25.00-mL of 0.002517 M K2C12O7 resulted in the reaction6 Fe2* + Cr2O7?- + 14 H* → 6 Fe³+ + 2 Crt + 7 H2OThe excess K2Cr2O7 was back-titrated with 8.53 mL of 0.00949 M Fe² solution. Calculatethe concentration of iron in the sample in parts per million.

Balanced equation of the reaction between Fe2+ and Cr2O72- indicates 6 moles of Fe2+ combines with 1…

A 100.0-mL sample of spring water was treated to convert any iron present to Fe2*. Addition of 25.00-mL of 0.002517 M K2C12O7 resulted in the reaction 6 Fe²* + Cr2O7²- + 14 H* → 6 Fe* + 2 Cr³+ + 7 H;O The excess K:Crz07 was back-titrated with 8.53 mL of 0.00949 M Fe²* solution. Calculate the concentration of iron in the sample in parts per million.

A 100.0-mL sample of spring water was treated to convert any iron present to Fe2. Addition of 25.00-mL of 0.002517 M K2C12O7 resulted in the reaction 6 Fe² + Cr2O7²- + 14 H* → 6 Fe* + 2 Cr³+ + 7 H;O The excess K:Crz07 was back-titrated with 8.53 mL of 0.00949 M Fe²* solution. Calculate the concentration of iron in the sample in parts per million.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section4.9: Spectrophotometry

Problem 2.1ACP: Excess KI is added to a 100.0-mL sample of a soft drink that had been contaminated with bleach,...

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