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- Part I. You considered the equilibrium: Fe3+(aq) + SCN-(aq) Fe(SCN)2+(aq), and compared the color of the solutions in four test tubes.
- In the first test tube, you added 1.0 mL of 0.1 M Fe(NO3)3.
- What color change was observed and what did this color change indicate about the shift in equilibrium?
- a. The solution turned yellow indicating that the equilbrium shifted to the left increasing [Fe3+] and [SCN-], as well as, decreasing the [Fe(SCN)2+].
- b. The solution turned yellow indicating that the equilbrium shifted to the left decreasing [Fe3+] and [SCN-], as well as, increasing the [Fe(SCN)2+].
- c. The solution turned deep red indicating that the equilbrium shifted to the right increasing [Fe3+] and [SCN-], as well as, decreasing the [Fe(SCN)2+].
- d. The solution turned deep red indicating that the equilbrium shifted to the right decreasing [Fe3+] and [SCN-], as well as, increasing the [Fe(SCN)2+].
- e. No color change was observed indicating that equilibrium was unaffected.
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