Soln. 2.5x10-3 M Fe(NO3)3 mL 2.5X10-3 M KSCN mL 0.5 M HNO3 mL Absorbance A 5...
| Soln. | 2.5x10-3 M Fe(NO3)3 mL | 2.5X10-3 M KSCN mL | 0.5 M HNO3 mL | Absorbance |
| A | 5 | 1 | 4 | 0.020 |
| B | 5 | 2 | 3 | 0.034 |
| C | 5 | 3 | 2 | 0.037 |
| D | 5 | 4 | 1 | 0.056 |
| E | 5 | 5 | 0 | 0.066 |
Calibrated at max wavelength of FeSCN2+ = 485.80nm
Final concentration of Fe3+ = 5.56*10-5
- Using M1V1=M2V2, calculate the initial concentrations of the reactant Fe3+, (m) and SCN- (n) in each solution A-E.
Homework Answers
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Soln.
2.5x10-3 M Fe(NO3)3 mL
2.5X10-3 M KSCN mL
0.5 M HNO3 mL
Absorbance
A
5...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution KSCN (mL) Fe(NO3)3 (mL) 0.5 5 [FeSCN2+] (mol/L)* 1 4.0x10^-5 Add 1.0 M 2 1.0 5 8.0x10^-5 HNO3 3 1.5 5 1.2x10^-10 4 2.0 5 1.6x10-4 to each to adjust the volume to 25 mL. 5 2.5 5 2.0x10-4 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2+] (in Soln 1) = [SCN-]...
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of...
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M. Part A: Calculate the number of moles of Fe3+ initially added to the solution. Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium....
Table A. Preparation of Standard solutions of FeSCN2+ 0.002 M 0.200 M 1.0 M HNO3 [FeSCN2+]...
Table A. Preparation of Standard solutions of FeSCN2+ 0.002 M 0.200 M 1.0 M HNO3 [FeSCN2+] (mol/L)* Solution KSCN (mL) Fe(NO3)3 (mL) 1 0.5 5 Add 1.0 M 1.0 5 N HNO3 3 1.5 5 4 2.0 5 to each to adjust the volume to 25 mL. 5 2.5 5 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2-] (in Soln 1) = [SCN-] (in Soln 1). The same...
5.0 mL of 0.0020 M Fe(NO3)3 was mixed with 3.0 mL of 0.0020 M KSCN and...
5.0 mL of 0.0020 M Fe(NO3)3 was mixed with 3.0 mL of 0.0020 M KSCN and 2.0 mL of. The absorbance of this solution at 447 nm was measured as 0.35. A calibration curve was created using four standard solutions of Fe(SCN)2+. The equation for the best-fit line of [FeSCN2+] vs Abs was y = 5025x + 0.004. Using the data provided, calculate an equilibrium constant (Kc) for the formation of [Fe(SCN)2+]. For the above reaction, how were we able...
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Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL 2.00 × 10−3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28 × 10−4 M. Find Kc for the reaction Fe3+(aq) + SCN−(aq) ↔ FeSCN2+(aq). a. What is the initial concentration of Fe3+ in the reaction mixture? [Fe3+] = ___ x 10-3 M b. What is the initial concentration of SCN- in the reaction mixture? [SCN-] = ___...
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A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C.
A student mixes 5.12 mL of 4.02 x 10...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution KSCN (mL) Fe(NO3)3 (mL) 0.5 5 [FeSCN2+] (mol/L)* 1 4.0x10^-5 Add 1.0 M 2 1.0 5 8.0x10^-5 HNO3 3 1.5 5 1.2x10^-10 4 2.0 5 1.6x10-4 to each to adjust the volume to 25 mL. 5 2.5 5 2.0x10-4 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2+] (in Soln 1) = [SCN-]...
Table A. Preparation of Standard solutions of FeSCN2+ 0.002 M 0.200 M 1.0 M HNO3 [FeSCN2+] (mol/L)* Solution KSCN (mL) Fe(NO3)3 (mL) 1 0.5 5 Add 1.0 M 1.0 5 N HNO3 3 1.5 5 4 2.0 5 to each to adjust the volume to 25 mL. 5 2.5 5 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2-] (in Soln 1) = [SCN-] (in Soln 1). The same...
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A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C.
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