Refer to Table 2, test solution 3 in the procedure. At equilibrium, the concentration of the FeNCS2+ is determined to be 1.5 x 10-4 M in 10.0 mL total volume of solution. a. Calculate the number of moles of Fe3+ and SCN- added. b. Calculate the number of moles of FeSCN2+ formed. c. Calculate the number of moles of each reactant present at equilibrium. moles at equilibrium = initial moles - moles used up d. Calculate the concentrations of all species at equilibrium. e. Calculate K.

Refer to Table 2, test solution 3 in the procedure. At equilibrium, the concentration of the FeNCS2+ is determined to be 1.5 x 10-4 M in 10.0 mL total volume of solution. a. Calculate the number of moles of Fe3+ and SCN- added. b. Calculate the number of moles of FeSCN2+ formed. c. Calculate the number of moles of each reactant present at equilibrium. moles at equilibrium = initial moles - moles used up d. Calculate the concentrations of all species at equilibrium. e. Calculate K.

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter13: An Introduction To Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 13.11QAP: The equilibrium constant for the conjugate acid-base pair HIn+H2OH3O++In is 8.00 10-5. From the...

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