For the solutions that you will prepare in Step 1 (Part 1) below, calculate the

Question

For the solutions that you will prepare in Step 1 (Part 1) below, calculate the [FeSCN^2+]. Presume that all of the SCN^- ions react. In Part 1 of the experiment, mol of SCN^- = mol of FeSCN^2+. Thus, you can calculate [FeSCN^2+] using the dilution equation, M_1V_1 = M_2V_2, the concentration of SCN^-, the volume of SCN^-, and the total volume of solution. Part 1 - Prepare and Test Standard Solutions Label five 100 mL beakers 1-5. In three other small beakers, obtain small volumes of: 0.200 M Fe(N0_3)_3, 0.0020 M SCN^-, and distilled water. CAUTION: Fe(N0_3)_3 solutions in this experiment are prepared in 1.0 M HNO_3 and should be handled with care. Prepare the first solution using a 10.0 mL pipet and a pipet filler. Measure the amounts of each reactant given into a 50 mL volumetric flask and then fill to line with distilled water. Mix each solution thoroughly in the volumetric flask and then pour into one of the labelled 100 mL beakers. Rinse the volumetric flask with distilled water, and then make the next solution. Continue until all 5 solutions have been made. Measure and record the temperature of one of the five solutions to use as the temperature for the equilibrium constant, K_eq.

Explanation / Answer

beaker number 0.2 M Fe(NO3)3 (ml) 0.002 M SCN- (ml) [FeSCN2+] in Molar 1 5.0 0.0 0.0 M 2 5.0 2.0 5.714 * 10-4 M 3 5.0 3.0 7.5 * 10-4 M 4 5.0 4.0 8.88 * 10-4 M 5 5.0 5.0 10 * 10-4 M

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.