A student mixed 5.00mL of 0.0020M Fe(NO3)3, 3.00mL of 0.0020M KSCN, and 3.00mL of distilled water. The mixture reacted to form a reddish solution indicating that FeSCN2+ was formed, according to the equation below. An absorbance of 0.21 was measured for this solution in a Spectrophotometer set at a wavelength of 447nm. Fe³+ (aq) + SCN (aq) → FeSCN²+ (aq) A calibration curve was used to find the equilibrium concentration of the product of this reaction: y = 1895x + 0.027 Calculate the equilibrium concentration of the Fe³+ Report your answer to 4 sig figs

A student mixed 5.00mL of 0.0020M Fe(NO3)3, 3.00mL of 0.0020M KSCN, and 3.00mL of distilled water. The mixture reacted to form a reddish solution indicating that FeSCN2+ was formed, according to the equation below. An absorbance of 0.21 was measured for this solution in a Spectrophotometer set at a wavelength of 447nm. Fe³+ (aq) + SCN (aq) → FeSCN²+ (aq) A calibration curve was used to find the equilibrium concentration of the product of this reaction: y = 1895x + 0.027 Calculate the equilibrium concentration of the Fe³+ Report your answer to 4 sig figs

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...

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Question

A student mixed 5.00mL of 0.0020M Fe(NO3)3, 3.00mL of 0.0020M
KSCN, and 3.00mL of distilled water. The mixture reacted to form a
reddish solution indicating that FeSCN2+ was formed, according to
the equation below. An absorbance of 0.21 was measured for this
solution in a Spectrophotometer set at a wavelength of 447nm.
Fe³+ (aq) + SCN (aq) FeSCN2+ (aq)
A calibration curve was used to find the equilibrium concentration of
the product of this reaction: y = 1895x + 0.027
Calculate the equilibrium concentration of the Fe³+ Report your
answer to 4 sig figs

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