Why is a large excess of Fe3+ added when preparing the standard solution. Why do you not add a large excess of Fe3+ when preparing the equilibrium solution. Fe^3+ + SCN^- = FeSCN^2+?
Why is a large excess of Fe3+ added when preparing the standard solution. Why do you...
Why is a large excess of Fe3+ added when preparing the standard solution. But you not add a large excess of Fe3+ when preparing the equilibrium solution. Fe^3+ + SCN^- = FeSCN^2+
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...
Fe3+ (aq) + ow does the equilibrium shift a) if you add more Fe* SCN (aq) = FeSCN2+ (aq) Fes b) if you remove SCN c) if you remove FeSCN+2 d) if you add more Fe" and you remove FeSCN2 e) if you remove Fe" and you remove FeSCN+2
Why is HCl added when preparing a stock solution of 10mM Fe3+? (1.62g of FeCl3 and 2ml of HCL stock solution is mixed and filled up to 1L with distilled water)
Doing a Chem Review, these are just study scenarios that I need to have a good understanding of 6. To determine the concentration of SCN in our saliva, we reacted the SCN in the saliva with Fe' according to the following reaction: We measured the absorbance of the FeSCN and used the absorbance value of the FesCN2 to obtain the concentration of the FesCN2*. This was achieved by measuring the absorbance values of standard FeSCN2+ solutions and constructing a calibration...
As you will do in lab, a student prepared the following 2 mixtures and recorded their absorbances in a cuvette with a 1.00 cm path length Table 1.Absorbance of iron (Il) thiocyanate Volume, ml Fe3- 10.0 0.020 M2.64 x 10M Absorbance SCN 10.0 10.0 Mix #1 0.20 M Fel 10.01 0.769 0.495 1. Write the balanced equilibrium reaction of Fe(aq) with SCN (aq) to form [FeSCNJ (aq). 2. Write the equilibrium formation constant expression for the reaction (Kyexpression) Determination of...
Lab Report: Determination of Kc for a Complex Ion Formation tube 2.00e-3 Fe3+ (mL) 2.00E-3M SCN- (mL) water (mL) initial conc. Fe3+ initial conc. SCN- 1 5.00 5.00 0 1.00e-3M 1.00E-3M 2 5.00 4.00 1.00 1.00E-3M 8.00E-3M 3 5.00 3.00 2.00 1.00E-3, 6.00E-3M 4 5.00 2.00 3.00 1.00E-3M 4.00E-3M 5 5.00 1.00 4.00 1.00E-3M 2.00E-3M 10ml of 0.200M Fe3+, 2.00ml of 0.00200M SCN-, AND 8.00ml of water results in an eq. [FeSCN2+] IN Standard Soln.:2.00E-4M Could you please explain how...
Iron thiocyanate (FeSCN2+) is a complex ion that appears orange-red in solution. Iron(III) (Fe3+) and thiocyanate (SCN-) are both colorless in solution. FeSCN2+ (aq) --(equilibrium)-- Fe3+ (aq) + SCN- (aq) a) If you add Fe(NO3)3 to a solution of these ions at equilibrium, in which direction will the reaction run to reach a new equilibrium? b) Silver ions react with thiocyanate ions to form a white precipitate. If you add silver ions to a solution of these ions at equilibrium,...
In the calibration solutions, the very large excess of Fe3+ ion compared to the amount of NCS- ion used to prepare the the mixtures allows us to make what assumption about the concentration of product in the mixtures? Question 8 options: [Fe(NCS)2+]equilibrium = [NCS-]equilibrium [Fe(NCS)2+]equilibrium = [Fe3+]initial [Fe(NCS)2+]initial = [Fe3+]initial [Fe(NCS)2+]equilibrium = [Fe3+]equilibrium [Fe(NCS)2+]equilibrium = [NCS-]initial [Fe(NCS)2+]initial = [NCS-]initial
A flask contains this equilibrium Fe3+(aq) + SCN'-(aq) <======> FeSCN'-(aq) Which direction should equilibrium shift when a few drops of iron(II) chloride is added? shift left no change b. shift right a. c.