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A standard solution of FeSCN2+ is prepared by combining 9.0 mL of 0.20 M Fe(NO,), with 1.0 mL of 0.0020 M KSCN. The...
Question 6 of 10 > A standard solution of FeSCN2 is prepared by combining 9.0 mL...
Question 6 of 10 > A standard solution of FeSCN2 is prepared by combining 9.0 mL of 0.20 M Fe(NO), with 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO), + KSCN = FeSCN2+ + KNO, +2 NO; What allows us to assume that the reaction goes essentially to completion? The concentration of Fe(NO), is much higher than the concentration of KSCN. The excess Fe* prevents the formation of the neutral Fe(SCN), The reaction...
Resume < Question 6 of 10 > Attempt 1 - A standard solution of FeSCN is prepared by combining 9.0 ml of 0.20...
Resume < Question 6 of 10 > Attempt 1 - A standard solution of FeSCN is prepared by combining 9.0 ml of 0.20 M Fe(NO), with 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO3), + KSCN = FeSCN2+ + KNO, +2 NO; What allows us to assume that the reaction goes essentially to completion? The concentration of Fe(NO,), is much higher than the concentration of KSCN. The excess Fe" prevents the formation of...
0.0018 is a wrong answer. Please do it again. Question 6 of 10 Try Again > Attempt 3 A standard solution of FeSCN...
0.0018 is a wrong answer. Please do it again.
Question 6 of 10 Try Again > Attempt 3 A standard solution of FeSCN2+ is prepared by combining 9.0 mL of 0.20 M Fe(NO3), with 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO3)3 + KSCN=FeSCN2+ + KNO, +2 NO; What allows us to assume that the reaction goes essentially to completion? The concentration of Fe(NO,), is much higher than the concentration of KSCN. The...
Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0...
Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0 ml of 0.20 M Fe(NO) with I.0 mL of 0.0020 M KSCN. The standard solution had an absorbance of 0.540. Fe* (ag)+SCN (ag)FeSCN*(a) A trial solution was made in a similar manner, but with a more dilute Fe(NO,), reagent. The initial SCN" concentration. immediately after mixing, was 0.00060 M. This trial solution had absorbance of 0.250. What is the equilibrium concentration of SCN in...
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...
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....
A mixture is prepared by combining 10.20 mL of 1.80 x 10-3 M Fe(NO3)3 with 10.00...
A mixture is prepared by combining 10.20 mL of 1.80 x 10-3 M Fe(NO3)3 with 10.00 mL of 1.68 x 10-3 M KSCN. The solution turns red due to the formation of FeSCN2+. The absorbance is measured and, using a calibration plot, the [FeSCN2+] at equilibrium is found to be 2.20 x 10-4 M. Complete the following ICE table Fe3+ + SCN- ⇌ FeSCN2+ initial (M) (A) (B) (C) change (M) (D) (E) (F) equilibrium (M) (G) (H) (I) What...
For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to...
For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to a volume of 450.0 ml, then... 4.00 mL of the diluted Fe(NO3)3 were mixed with 4.00 mL of KSCN and 4.00 mL of HNO3. Calculate the initial concentration of Fe3+ at the time of mixing. Short answer LE- _ (no extra Scientific notation format spaces) How many mL of 0.00200 M Fe(NO3)3 are required to prepared 12.50 mL total volume with a concentration of...
A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN.
A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN. The student finds that the equilibrium concentration of FeSCN2+ is 5.6 x 10-4M. a. Set up the Kc expression for the following equation. Fe3+ + SCN- ↔ FeSCN2+b. What is the total volume of the solution? _______ mL c. Fill in the following table for the moles of each species.d. Find the concentration for the above ions. e. Calculate Kc for the reaction.
Question 6 of 10 > A standard solution of FeSCN2 is prepared by combining 9.0 mL of 0.20 M Fe(NO), with 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO), + KSCN = FeSCN2+ + KNO, +2 NO; What allows us to assume that the reaction goes essentially to completion? The concentration of Fe(NO), is much higher than the concentration of KSCN. The excess Fe* prevents the formation of the neutral Fe(SCN), The reaction...
Resume < Question 6 of 10 > Attempt 1 - A standard solution of FeSCN is prepared by combining 9.0 ml of 0.20 M Fe(NO), with 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO3), + KSCN = FeSCN2+ + KNO, +2 NO; What allows us to assume that the reaction goes essentially to completion? The concentration of Fe(NO,), is much higher than the concentration of KSCN. The excess Fe" prevents the formation of...
0.0018 is a wrong answer. Please do it again.
Question 6 of 10 Try Again > Attempt 3 A standard solution of FeSCN2+ is prepared by combining 9.0 mL of 0.20 M Fe(NO3), with 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO3)3 + KSCN=FeSCN2+ + KNO, +2 NO; What allows us to assume that the reaction goes essentially to completion? The concentration of Fe(NO,), is much higher than the concentration of KSCN. The...
Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0 ml of 0.20 M Fe(NO) with I.0 mL of 0.0020 M KSCN. The standard solution had an absorbance of 0.540. Fe* (ag)+SCN (ag)FeSCN*(a) A trial solution was made in a similar manner, but with a more dilute Fe(NO,), reagent. The initial SCN" concentration. immediately after mixing, was 0.00060 M. This trial solution had absorbance of 0.250. What is the equilibrium concentration of SCN in...
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-]...
For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to a volume of 450.0 ml, then... 4.00 mL of the diluted Fe(NO3)3 were mixed with 4.00 mL of KSCN and 4.00 mL of HNO3. Calculate the initial concentration of Fe3+ at the time of mixing. Short answer LE- _ (no extra Scientific notation format spaces) How many mL of 0.00200 M Fe(NO3)3 are required to prepared 12.50 mL total volume with a concentration of...
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