For Part A of the Equilibrium experiment, you will be preparing several standard solutions for the...
Bienvenido a Trip.com In Part 1 of the lab you will make the following four solutions: About 3221 Solution Number 0.500 M Fe3+ 3.00 x 10-4 M SCN' water 2.50 mL 2.50 ml 2.50 mL 2.00 mL 0.50 mL 2.50 mL 1.50 mL 1.00 mL 2.50 mL 1.00 mL 1.50 mL 0 mL Given the data in the table above, determine the initial concentrations of [Fe3+] and [SCN"). Since one of the reactants is in excess, you can determine (FeSCN2+Jeg...
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. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you will prepare using the information in Table 2 Volume of delonged water (ml) Total volume ml) Table 2. Preparation of Equilibrium Mixtures Volume of Volume of Volume of 0.10 M Mixture 0.00200 M 0.00200 M HNO, (ml) KSCN (ML) Fe(NO3)3 (ml) 1,50 3.00 1.00 2.00 1.00 2.50 1.00 1.50 350 1.00 1.00 2.50 2.00 4.50 4.50 4.50 4.50 4.50 10.00 10.00 10.00 10.00 10.00...
5. In this experiment, you will prepare a standard solution for a calibration curve for the formation of FeSCN2 complex by reaction different volumes of 0.2 M Fe(NO,), and 0.002 M NaSCN. You will use 0.05M HNO, for all dilutions. Using the table, Calculate the equilibrium concentrations of FeSCN2 Vol of Fe Vol of SCN 0.1 M HNO Equilibrium concentration Fe[SCN]2' (mL) (mL.) (mL) 10.00 0.00 10.00 10.00 1.00 9.00 10.00 2.00 8.00 10.00 3.00 7.00 10.00 4.00 6.00 10.00...
For each equilibrium sample, calculate the initial concentrations (assuming no reaction occurred) of SCN– and Fe3+ based on the dilution factors used. Enter the absorbance values for each sample. For the standard solution, assume that, when equilibrium is reached, the [FeSCN2+]eq is equal to [SCN–]ini. Why is this a good assumption? For the equilibrium solutions, calculate the [FeSCN2+]eq (Ceq) using Eq. 4. Using Eq. 5 and 6, calculate [Fe3+(aq)]eq and [SCN–(aq)]eq for each equilibrium solution. Calculate values for the equilibrium...
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-] = 1.239; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.454 M. What is the numerical value of KC for this equilibrium? KC = __________________ 2) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.370; [SCN-] = 0.777; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.285 M. What is the equilibrium concentration of Fe3+? [Fe3+]eq =...
Use the following procedure for answering questions given below: 3.00 mL of 2.00 x 10' M solution of Fe(NO3)3 was mixed with 4.00 mL of 2.5 x 10-3 M solution of KSCN and 1.00 mL of 0.5M HNO3. After equilibrium: Fe3+ + SCN FeSCN2+ = was established the equilibrium concentration of FeSCN2+ ions was read from the calibration curve as 5.00 x 10-4 M. 01. The initial concentration of Fe3+ ions (assuming no reaction took place) was: [20] a) 1.00...
A student made solution #3 using the experimental method in this lab, and measured an absorbance of 0.559. The starting reagents are 2.00 x 10-3 M Fe(NO3)3 and 2.00 x 10-3 M KSCN. The amount of absorption is proportional to the concentration of FeSCN2+. This relationship – true for many solutions – is called “Beer’s Law”, and has the simple equation: A = bc where “A” is the absorption, “b” is 5174.6 for FeSCN2+ and “c” is molarity Make Five...
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...
Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL 2.00 × 10−3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28 × 10−4 M. Find Kc for the reaction Fe3+(aq) + SCN−(aq) ↔ FeSCN2+(aq). a. What is the initial concentration of Fe3+ in the reaction mixture? [Fe3+] = ___ x 10-3 M b. What is the initial concentration of SCN- in the reaction mixture? [SCN-] = ___...