EQUILIBRIUM OF A METAL COMPLEX ION Part 2: Determination of the Equilibrium Constant 1. Write the...
Can't figure out the concentration of the complex of
solns. 10, 11, 12, 13, & 14.
Modern Experimental Chemistry Chemistry 153 The Iron(III) Thiocyanate Complex Purpose of the Experiment To determine the chemical formula of a complex ion and measure its formation equilibrium constant Equipment Spectro Vis spectrophotometer and LabQuest, cuvette, 25-mL buret (3), ring stand, buret clamp (2), 50-mL beaker (3), small plastic beakers Reagents SCN, as KSCN, 0.00200 M solution Fe; as Fe(NO), 0.00200 M solution and a...
please correct me If I did anything wrong. im very confused on
this.
• Determining k in Beer's Law 2. Determining the equilibrium constant Test Tube No. Absorbance Test Tube No. Absorbance 0,060 이79 0.253 0319 0.400 0.120 0.268 0.361 0.461 0.695 Post Laboratory Questions 1. Complete the following table and calculate k-value for the Beer's Law. All concentrations should be in M. [Fe(SCN)2) Absorbance CA Test Tube No. Diluted Fe(NO3)2 (mL) 0 . 2 3 4 s Reference 1.0...
Name Equilibrium Constant Lab Prelab assignment 1. Determine the initial concentrations (in molarity) of Fe and SCN" after mixing in each of the 5 beakers in Part I. Then, calculate the [FeSCN2 1 assuming that the reaction goes to completion and that all of the SCN ions react. Show a sample calculation then put your answers in the box below. [FESCN2 Jeg Beaker number [Fe") [SCN' 2 3 4 5 2. In preparing the standard solutions for Part 1, the...
Write the expression for the equilibrium constant for the following reaction, Fe+3 (aq) + SCN- (aq) ↔ Fe(SCN) +2 (aq) The slope of the calibration curve of [Fe(SCN)+2] vs absorbance is 3.5 x 104 M-1. Given that the absorbance of the solution prepared using 5.0 mL from 0.002 M Fe+3 and 3.0 mL from 0.002 SCN- is 0.422. Calculate the equilibrium constant for this solution.
5. A student does an experiment to determine the equili but at a higher temperature. ermine the equilibrium constant for the same reaction that you will study, Fe** (aq) + SCN (aq) FeSCN2+ (aq) The student prepares solution 1, by mixing 5. s Solution, by mixing 5.00 ml of 0.002 M Fe(NO2)2 solution with 5.00 mL of .00011M KSCN solution, heats the mixture, and finds that the equilibrium concentration of F and finds that the equilibrium concentration of FeSCN2+ in...
I am doing a lab on the determination of the equilibrium constant for the formation of Fe(SCN)+2. We used a spectrometer to measure the absorption of solutions with a varying initial concentration of Fe+3, but constant concentrations of SCN-. The reaction equation of Fe+3 + SCN- —> Fe(SCN)+2. Along with the SCN- and Fe+3 stock solutions, we also combined them with .3 M HNO3. We then calculated an average molar absorptivity and the equilibrium concentration of Fe(SCN)+2. From that concentration...
values used for table 2
how do you do the Ice tables???
Experiment V. Equilibrium Constant Lab Report ( 50 pts) Calibration Curve 1. Record the absorbance for each of the standard solutions in the table below. Calculate the concentration of FeSCN)" in each of the standard solutions and record the values in the table below. Show a sample calculation (for A2) of your work in the space below the table. Solution Absorbance [Fe(SCN)" A-1 A-2 A-3 0.000 0.390 0.535...
Beers law solve for E3 and E4 showing work
Part II. Equilibrium Constant Calculations
Calculate the initial moles of Fe3+ and SCN- for solutions E2
through E6 and record these values in the table on your Data Sheet.
You obtain the moles of the reactants by multiplying their molarity
by the volume (in L) of their solution used.
Determine the equilibrium concentration of FeSCN2+ for each of
the solutions E2-E6 from your Beer’s Law plot. Using these
equilibrium concentrations, the...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part II (y values and the best-fit line equation from Part I to calculate the [FeSCN2"), at equilibrium. Show two sets of calculations and complete Table 6 below. Sample Calculation with hypothetical values of Absorbance from Table 4 & fitted egn. from Table 3 y = mx + b (y is absorbance) 0.0620 - 2000x -0.0250 x-0.0620+ 0.0250 2000 = 4.35 x 10 с D...
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...