Be sure to answer all parts. Commercial silver-plating operations frequently use a solution containing the complex Ag+ ion. Because the formation constant (Kf) is quite large, this procedure ensures that the free Ag+ concentration in solution is low for uniform electrodeposition. In one process, a chemist added 9.0 L of 5.0 M NaCN to 90.0 L of 0.17 M AgNO3. Calculate the concentration of free Ag+ ions at equilibrium. See your textbook for Kf values. × 10 M (Enter your answer in scientific notation.)
Be sure to answer all parts. Commercial silver-plating operations frequently use a solution containing the complex Ag+ i...
Commercial silver plating operations frequently use a solution containing the complex |Ag(CN)_2] ion. Because the formation constant K_f is quite large, this procedure ensures that the free Ag+ concentration in solution is low to promote uniform electrodeposition. In one process, a chemist added 9.0 L of 1.1M NaCN to 90.0 L of 0.12 M AgN0_3. Calculate the concentration of free Ag+ ions at equilibrium. K_f for this reaction is 1.0 times 10^21. Enter your answer in scientific notation.
i need help with this lab please. can i get someone to answer the entire thing. thank you Instructor Equilibria of Coordination Compounds OBSERVATIONS AND DATA 1. The formation of complex ions with ammonia The net ionic equation for the reaction of excess Cuso, with NH, is 24 Cu2+ + 4NH3 [cu (NH3)4] The predicted effect on the reaction above of adding excess NH, (based on Le Châtelier's principle) is The reaction will shift to the night and product formation...