Calculate the molarity of Fe3+ in solution A. Solution A: 10 mL of 0.0600 M Fe(No3)3 ...
Calculate the molarity of Fe3+ in solution A.
Solution A: 10 mL of 0.0600 M Fe(No3)3
+ 15 mL DI water.
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Calculate the molarity of Fe3+ in solution A.
Solution A: 10 mL of 0.0600 M Fe(No3)3 ...
A student took 5.03 mL 0.200 M Fe(NO3)3 solution, added 25.18 mL of DI water, mixed the resulting solution thoroughly and placed the solution in a 50 mL buret. Then, the student took 10.09 mL of this...
A student took 5.03 mL 0.200 M Fe(NO3)3 solution, added 25.18 mL of DI water, mixed the resulting solution thoroughly and placed the solution in a 50 mL buret. Then, the student took 10.09 mL of this dilute solution from the buret and mixed it thoroughly with 6.21 mL 0.00200 M NH4SCN and 28.65 mL DI water to form the reaction system. What are the initial [Fe3+] and the initial [SCN-] in this reaction system? ( ) [Fe3+]Initial = 7.47...
a. A 10 ml calibration solution is made by mixing 5 mL of 0.200 M Fe(NO3)3,...
a. A 10 ml calibration solution is made by mixing 5 mL of 0.200 M Fe(NO3)3, 1.50 mL of 2.00X10-3 M KNCS, 1 mL of 0.100 M nitric acid and 2.50 mL H20. What is the final concentration of only the NCS-ion? b. If 1.00 ml of this solution is then diluted to a final volume of 25.00 ml with DI water. What is the new concentration of NCS?
5.00 mL of 5.00 × 10-1M Fe(NO3)3 are mixed with 2.00 mL of 1.00 x 10-4M NASCN and 3.00 mL of 0.5M HNO3
5.00 mL of 5.00 × 10-1M Fe(NO3)3 are mixed with 2.00 mL of 1.00 x 10-4M NASCN and 3.00 mL of 0.5M HNO3. A. Calculate the molarity of the Fe3+ in the diluted solution. B. Calculate the molarity of the SCN in the diluted solution. C. Assume that the following reaction goes to completion: Calculate the molarity of the FeSCN2+ in the diluted solution.
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 student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x...
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...
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...
Part A of lab: pour 30 ml of 0.150 M Fe(NO3)3 into a 50 ml beaker...
Part A of lab: pour 30 ml of 0.150 M Fe(NO3)3 into a 50 ml beaker and pipette 10 ml of this solution into a 25 ml volumetric flask. This is the standard reagent blank Part B of lab: pour 30 ml of 1.50*10^-3 M Fe(NO3)3 into a 25 ml volumetric flask. This is the reagent blank. Why is a large excess of Fe3+ added to make the standard solution, and why do you NOT add a large excess of...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250 M NaSCN, the following reaction occurs: Fe3+ (aq) + SCN(aq) $ FeSCN2+(aq) At equilibrium the concentration of FeSCN2- is found to be 6.00 x 10-2 M. A. Fill in the table below with the proper numerical values. (Remember to take into account the effects of dilution when calculating the initial molarity of Fe3+ (aq) and SCN'(aq) Fes- (aq) SCN (aq) FeSCN-(aq) Initial Molarity Change...
What is the concentration of Fe3+ in a solution of 1.5 mL of 0.020 M KI,...
What is the concentration of Fe3+ in a solution of 1.5 mL of 0.020 M KI, 2.5 mL of 0.020 M Fe(NO3)3, and 6.0 mL of water?
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.
a. A 10 ml calibration solution is made by mixing 5 mL of 0.200 M Fe(NO3)3, 1.50 mL of 2.00X10-3 M KNCS, 1 mL of 0.100 M nitric acid and 2.50 mL H20. What is the final concentration of only the NCS-ion? b. If 1.00 ml of this solution is then diluted to a final volume of 25.00 ml with DI water. What is the new concentration of NCS?
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...
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...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250 M NaSCN, the following reaction occurs: Fe3+ (aq) + SCN(aq) $ FeSCN2+(aq) At equilibrium the concentration of FeSCN2- is found to be 6.00 x 10-2 M. A. Fill in the table below with the proper numerical values. (Remember to take into account the effects of dilution when calculating the initial molarity of Fe3+ (aq) and SCN'(aq) Fes- (aq) SCN (aq) FeSCN-(aq) Initial Molarity Change...
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