One drop of 2.5 M KSCN solution is added to 0.5 mL of 0.10 M Fe(NO3)3. After the solution is mixed, 1.0 mL of 0.125 M EDTA solution is added. Enter the chemical formula of the major iron complex in solution after the addition of EDTA
Ans :- Chemical formula of the major iron complex is Fe(EDTA)3
Explanation :-
When KSCN and Fe(NO3)3 are mixed the chemical equation is :
Fe(NO3)3 (aq) + KSCN (aq) --------------> Fe(SCN)3 (aq) + KNO3 (aq)
After the addition of EDTA :-
| Fe(SCN)3 (aq) + 3 EDTA- (aq) -----------------> Fe(EDTA)3(s) + 3 SCN- (aq) |
One drop of 2.5 M KSCN solution is added to 0.5 mL of 0.10 M Fe(NO3)3. After the solution is mixed, 1.0 mL of 0.125 M ED...
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...
Given that the volume of one drop is approximately 0.05 mL, compare the number of moles for each ligand when one drop of 2.5 M KSCN is added to a test tube and 1.0 mL of 0.125 M EDTA added. Enter the number of moles of each ligand. Support your answers with appropriate calculations. Moles SCN− : Moles EDTA:
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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 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.
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....
If NH3 (ammonia, pKb=4.74) is added to a solution of Fe(NO3)3 such that right after the addition we have 50 mL of 5.0 M NH3 and 0.0040 M Fe(NO3)3 (right after addition) Find Kc for Fe2+(aq) + 2OH-(aq) ---> Fe(OH)2 (s) any type of explanation would be helpful please!
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