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11 Nov 2019
I'm having trouble with doing the assignment in the box correctly. Can anyone help me out? thank you!
Spectrometric Determination of the Equilibrium Constant for the Formation of [FeSCN]2+ revised by Bruce E. Wilcox, Fall 2015 Assignment: Do these problems in your lab.notebook AND paper to be banded in. SHOW WORK CLEARLY. All quantities must have detailed units. 1. What is the concentration of iron(111) ion in a solution made by taking 10.00 mL of a 0.300 M Fe solution and diluting it to the mark in a 100.0 mL volumetric flask? 2. What is the concentration of iron(III) ion in a solution made by taking 4.00 mL of the dilute solution made in question 1 and adding 6.00 mL of water to it? You can assume the volumes will add exactly 3. The source of the thlocyanate lon in this experiment may be from ammonium thiocyanate, potassium thiocyanate or sodlum thiocyanate. Why can we use any of these compounds? Introduction This experiment will investigate a simple equilbrium system to give you experience at collectingFigure 8. A hydrated iron(III) ion and processing data to determine the equilibrium constant for the system. The chemical system to be used is the complexation of one thiocyanate ion (SCN") to an aqueous Iron(III) lon by replacement of one of the coordinated water molecules in the hydrated iron(III). (Recall that transition metal ions exist in aqueous solution as hydrated ions, those with ypically six water molecules bonded to the iron(III) ion hrough lone pairs of electrons on the water molecules, gure 8.) The thiocyanate ion also has a lone pair of
I'm having trouble with doing the assignment in the box correctly. Can anyone help me out? thank you!
Spectrometric Determination of the Equilibrium Constant for the Formation of [FeSCN]2+ revised by Bruce E. Wilcox, Fall 2015 Assignment: Do these problems in your lab.notebook AND paper to be banded in. SHOW WORK CLEARLY. All quantities must have detailed units. 1. What is the concentration of iron(111) ion in a solution made by taking 10.00 mL of a 0.300 M Fe solution and diluting it to the mark in a 100.0 mL volumetric flask? 2. What is the concentration of iron(III) ion in a solution made by taking 4.00 mL of the dilute solution made in question 1 and adding 6.00 mL of water to it? You can assume the volumes will add exactly 3. The source of the thlocyanate lon in this experiment may be from ammonium thiocyanate, potassium thiocyanate or sodlum thiocyanate. Why can we use any of these compounds? Introduction This experiment will investigate a simple equilbrium system to give you experience at collectingFigure 8. A hydrated iron(III) ion and processing data to determine the equilibrium constant for the system. The chemical system to be used is the complexation of one thiocyanate ion (SCN") to an aqueous Iron(III) lon by replacement of one of the coordinated water molecules in the hydrated iron(III). (Recall that transition metal ions exist in aqueous solution as hydrated ions, those with ypically six water molecules bonded to the iron(III) ion hrough lone pairs of electrons on the water molecules, gure 8.) The thiocyanate ion also has a lone pair of
Deanna HettingerLv2
11 Nov 2019