2. We have a mixture of 100 mL of Fe³+ solution (1.00 × 103 M) and 100 mL of A ion solution (1.00 × 10-3 M). The mixture has a deep blue color, indicating the formation of a complex between Fe³+ and A- . From spectrophotometric analysis, we find that 30.0% of the Fe³+ is in the form of a complex, where there are two probable formulae: FeX2+ or FeX3. a. Balance the following equations and calculate the concentrations of the remaining species. Fe³+ +A=FeA²+, Fe³+ +AFEA. 4 After reaching equilibrium states, write the equilibrium expressions and the equilibrium constants for both cases in (a). b.
2. We have a mixture of 100 mL of Fe³+ solution (1.00 × 103 M) and 100 mL of A ion solution (1.00 × 10-3 M). The mixture has a deep blue color, indicating the formation of a complex between Fe³+ and A- . From spectrophotometric analysis, we find that 30.0% of the Fe³+ is in the form of a complex, where there are two probable formulae: FeX2+ or FeX3. a. Balance the following equations and calculate the concentrations of the remaining species. Fe³+ +A=FeA²+, Fe³+ +AFEA. 4 After reaching equilibrium states, write the equilibrium expressions and the equilibrium constants for both cases in (a). b.
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:2. We have a mixture of 100 mL of Fe³+ solution (1.00 x 10-3 M) and 100 mL of A ion solution (1.00 x
103 M). The mixture has a deep blue color, indicating the formation of a complex between Fe³+ and A-
. From spectrophotometric analysis, we find that 30.0% of the Fe³+ is in the form of a complex, where
there are two probable formulae: FeX²2 or FeX;.
Balance the following equations and calculate the concentrations of the remaining species.
Fe³+ +A¯=FeA²+,
Fe³+ +A
W
After reaching equilibrium states, write the equilibrium expressions and the equilibrium constants
for both cases in (a).
a.
b.
FeA3.
81
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