The sketch of the photometric titration curve for the titration of Iron(III) with Fe ( SCN ) 2+ is to be drawn, also explain the reason for using the green filter. Concept introduction: The photometric titration curve is the plot showing the relationship between the absorbance of the solution corrected for the particular volume changes versus the volume of the titrant present in the solution.

Question

A spectrophotometric method for the determination of Fe (II) is based on the measurement of the red-orange color of its complex with o-phenanthroline. The complex obeys Beer's law for Fe (II) concentrations lower than 9 ppm. It is known that a solution containing 0.100 ppm of Fe(II) in excess of o-phenanthroline produces an absorbance of 0.200 in a cuvette with 1.00 cm of optical path and that an unknown sample gives an absorbance of 0.470 under the same conditions, Calculate: a) The concentration of Fe in the unknown sample in moles/L and ppm. b) The molar absorptivity coefficient of the complex. Fact. Fe = 55.845

Answer 1

Question

Chapter 14, Problem 14.4QAP

Interpretation Introduction

Interpretation:

The sketch of the photometric titration curve for the titration of Iron(III) with Fe(SCN)2+ is to be drawn, also explain the reason for using the green filter.

Concept introduction:

The photometric titration curve is the plot showing the relationship between the absorbance of the solution corrected for the particular volume changes versus the volume of the titrant present in the solution.

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A spectrophotometric method for the determination of Fe (II) is based on the measurement of the red-orange color of its complex with o-phenanthroline. The complex obeys Beer's law for Fe (II) concentrations lower than 9 ppm. It is known that a solution containing 0.100 ppm of Fe(II) in excess of o-phenanthroline produces an absorbance of 0.200 in a cuvette with 1.00 cm of optical path and that an unknown sample gives an absorbance of 0.470 under the same conditions, Calculate: a) The concentration of Fe in the unknown sample in moles/L and ppm. b) The molar absorptivity coefficient of the complex. Fact. Fe = 55.845

1.Solution of EDTA is particularly valuable as titrants because the reagent combines with metal ions in a 1:1 ratio regardless of the charge on the cation. For example, Fe(ll) and Fe(ll), complexes are formed with EDTA with great stability. The formation constants for the Fe(ll)-EDTA chelate, and Fe(lll)-EDTA chelate are 2.1 x 1014 and 1.3 X 1025, respectively. a) For each ion complex mentioned above, write the equations of reactions for complex formation and expression for the complex formation constant. b) Calculate the concentration of Fet In a solution that was prepared by mixing 50.0 mL of 0.200 M Fohwith 200 0 o/oro.0100 M EDTA. The mixture was buffered to a ph of 11.00, (Given the valio of a, 0.85 al pH I1.00)

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