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 the reaction mixture
.
A student working in the laboratory prepared the following reactants: 5 mL of 0.007M Cd2+(aq) 10...
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...
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+...
Standard solutions of [Fe(SCN)2-] were prepared and their absorbance measured in order to study the Keq for the reaction Fe3+ + SCN- <=> FeNCS2+ A plot of absorbance verses concentration of [Fe(SCN)2-] is shown below. To determine the Keq for the above reaction, 10.00 mL of 0.00200 M Fe(NO3)3 solution is mixed with 5.00 mL of 0.0020 M KSCN and diluted with 5.0 mL 0f 0.10 M HNO3. The absorbance of this red solution is found to be 0.322....
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...
urgentt 5) The molecular complex Cd(CN)d-dissociates in water by the process Ca(CN)"(aq) = Cd2+(aq) +4 CN- Kc = 1.3 x 10-7 The initial concentration of Cd(CN).- in an aqueous solution is 0.0360 M. No Cd2+ or CN-ions are initially present. What is the concentration of Cd2+ ion present when equilibrium is achieved? [12 points]
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...