What is the initial [SCN-],M ? What is the Equilibrium [FeNCS2+],M?
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Suppose a solution could be made with the following ionic species concentrations at 25°C: [Fe3+] = 0.0015 M, [SCN-] = 0.0010 M, and [FeSCN2+] = 0.00080 M. Using the results of your experiment, determine whether this system is at equilibrium or, if not, in which direction the reaction would spontaneously proceed. Would the intensity of the color of the solution increase or decrease as equilibrium was approached? Explain. A water sample is to be tested for the presence of Fe3+ ions. To 10.0 mL of water is added some nitric acid and a high concentration of SCN-, resulting in a new total volume of 15.0 mL. The solution becomes slightly red in color. The %T at the wavelength used in this experiment was found to be 85.6%. From this information, and using your experimentally determined molar absorptivity ε, determine the molarity and ppm of Fe3+ in the sample.
Adi S.
2) A calibration solution contains 1.50 mL of 0.00200 M NaSCN, 5.00 mL of 0.200 M FeCl3, and enough 0.100 M HNO3 to make a total volume of 25.0 mL. Assuming that [Fe3+] is sufficient to drive the reaction to completion, what is the concentration of FeSCN2+ in this solution? (Answer: 1.20 x 10-4 M) 3) A student prepares an equilibrium solution by mixing 5.00 mL 0.00200 M Fe3+, 2.00 mL 0.00200 M SCN-, and 3.00 mL 0.100 M HNO3. What are the initial concentrations of Fe3+ and SCN- in this solution? (Answers: [Fe3+] = 1.00 x 10-3; [SCN-] = 4.00 x 10-4)
Dinesh S.
What is the value of the concentration of the SCN? Suppose the Keq for this experiment is 523. The initial concentration of the Fe3+ is 4.00 x 10^-2 M. The initial concentration of the SCN- is 1.00 x 10^-3 M. The reaction for the experiment is: Fe3+ + SCN- = Fe(NCS)2+. The concentration of the SCN- at equilibrium is Y x 10^-4 M. Your answer should have 2 significant figures.
David C.
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