A student working in the laboratory prepared the following reactants:
5 mL of 0.005M Cd2+(aq)
10 mL of 0.007M SCN-(aq)
10 mL of 0.8M HNO3(aq)
These reagents were mixed and allowed to stand for 10 minutes. The concentration of Cd(SCN)+ in the resulting equilibrium mixture is found to be 5 x 10−4M. Calculate the initial concentration of Cd2+(aq).
Calculate the equilibrium concentration of Cd2+(aq).Calculate the initial concentration of SCN-(aq).
Calculate the equilibrium concentration of SCN-(aq).
Calculate the Keq for the reaction mixture
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A student working in the laboratory prepared the following reactants: 5 mL of 0.005M Cd2+(aq) 10...
A student working in the laboratory prepared the following reactants: 5 mL of 0.007M Cd2+(aq) 10 mL of 0.005M SCN-(aq) 10 mL of 0.9M HNO3(aq) These reagents were mixed and allowed to stand for 10 minutes. The concentration of Cd(SCN)+ in the resulting equilibrium mixture is found to be 5 x 10−4M. Calculate the initial concentration of Cd2+(aq). Calculate the initial concentration of SCN-(aq). Calculate the equilibrium concentration of Cd2+(aq). Calculate the equilibrium concentration of SCN-(aq). Calculate the Keq for...
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-] = ___...
4- (a) Calculate the concentration of Cd2+ ion in a solution prepared by mixing 2.0 mL of 1 M CA(NO3)2 solution with 1.0 L of 4.0 M NH3 solution. [Assume that the volume does not change after the addition of 2.0 ml of 1 M Cd(NO3)2] (b) Will you be able to see Ca(OH)2(6) precipitate in the solution? (Kr for Ca(NH3)42+ = 1.0 x 107, Kb for NH3 = 1.8 x 10-5; Ksp for Ca(OH)2 = 5.9 x 10-15 Cd2+...
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...
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 25.0 mL volume of 0.0200 M Fe(NO3)3 is mixed with 50.0 mL of 0.00200 M NaSCN and 25.0 mL of 0.100 HNO3. The blood-red FeSCN2+ ion forms and the equilibrium is established: Fe3+(aq) + SCN-(aq) <---> FeSCN2+(aq) The equilibrium concentration of FeSCN2+ ([FeSCN2+]) was measured spectrophotometrically and found to be 7.0 x 10-4 mol/L. To calculate the equilibrium constant (Kc) for thr equilibrium system, proceed through the following steps: A. Moles of Fe3+, initial B. Moles of SCN-, initial...
A student mixed 4.00 mL of 1.02 x 10-1 M Fe(O3)3 with 100.0 mL of 1.98 x 10-4 M KSCN using 5.0 x 10-1 M HNO3 as the solvent for both solutions and found the absorbance of the resulting equilibrium mixture to be 0.235. Given these data, calculate the K value (The e value for Fe(SCN)2+ is 4700 L mole-1cm-1 and b = 1 cm) I got: [Fe^3+] = 3.87 x 10^-3 M [SCN^-] = 1.40 x 10^-4 M [Fe(SCN)^2+]...
1. A student mixes 5.00 mL of 2.00 x 10 M Fe(NO3)3 with 5.0 mL of 2.00 x 10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN+2 is 1.2 x 104 M. Find the Kc for the reaction of Fe (aq) + SCN (aq) → FeSCN2(aq) using the following steps. a. Find the initial concentration of Fe and SCN. (Use Equation 4). Record the value in the ICE Chart below. b. What is the equilibrium...
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...
G-10 Assume the equilibrium constant K 1 for a reaction A + B 2 C. You prepare a solution that has the following initial concentrations. For each solution, calculate the reaction quotient Q and state if the concentrations of reactants and products will (increase, decrease, or stay the same). a) [A] 1 M, [B] 1M, [C] 2 M. b) [A] 2 M, [B] 1 M,(C] 1 M. Answers: Q 4 >K, [A, B] increase, [C] decreases Q=0.5 < K, [A,...