What is the “free” silver ion concentration in a solution that was (pre-equilibrium) 0.10M AgNO3(aq) and 0.50M NH3(aq)? Kf for [Ag(NH3)2]+ = 1.7x107.
What is the “free” silver ion concentration in a solution that was (pre-equilibrium) 0.10M AgNO3(aq) and...
Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.140 M AgNO3 and 0.600 MNH3, and in which the following reaction takes place: Ag (ag)+2NH3 CaAg(NH3(aq) (K-1.7010) M Agt
please help What is the approximate concentration of free Cu* ion at equilibrium when 1.57x102 mol copperII) nitrate is added to 1.00 L of solution that is 1.380 M in NH3. For [Cu(NH3)4j2, Kf 2.1 1013 [Cu2 м What is the approximate concentration of free Fe2* ion at equilibrium when 1.42x102mol iron(II) nitrate is added to 1.00 L of solution that is 1.38so M in CN. For [Fe(CN)6]4, Kf=1.0x1035 [Fe"]= In the presence of excess OH, the Al*(aq) ion forms...
Determine the concentration of Ag+ in a solution prepared by adding 0.10 mol AgNO3 to 1.0 L of 3.5 M NH3. Ag+(aq) + 2 NH3(aq) left right double arrow Ag(NH3)2+(aq) Kf= 1.7 x 107
3. (4 pts) a) Decreasing the concentration of free metal ion in solution by complexing it was with a ligand will the solubility of an insoluble salt. b) [Ag] is a Lewis Ammonia is a Lewis c) Calculate [Ag*) at equilibrium when 0.220 M concentrated ammonia, NH3, is added to 0.020 M AgNO3. Assume AgNO3 dissociates completely. Neglect volume change.
Calculate the equilibrium molar concentration of free Zn2+(aq) in a solution that contains 0.021 mol of Zn2+ per liter to which 0.498 mole of NH3 is added. Kf for Zn(NH3)42+ is 2.9x109. Show the equilibrium equation.
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...
1- What is the approximate concentration of free Cu2+ ion at equilibrium when 1.71×10-2 mol copper(II) nitrate is added to 1.00 L of solution that is 1.310 M in NH3. For [Cu(NH3)4]2+, Kf = 2.1×1013. [Cu2+] = ------ M
Silver (I) ions in aqueous solutions react with NH3(aq) to form a complex ion according to the following reaction: Ag+ + 2NH3(aq) ---> Ag(NH3)2+ with a formation constant, Kf of 1.5 x 107. Calculate the solubility in g/L, of AgCN(s) (Ksp = 2.2 x 10-16) in 0.75M NH3(aq)
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...
Testbank, Question 17.074 In an aqueous solution silver ions can form Ag(NH3)2+(aq) in the presence of ammonia. For Ag(NH3)2+(aq): (see photo) Testbank, Question 17.074 In an aqueous solution silver ions can form Ag(NH3)2+ (aq) in the presence of ammonia. For Ag(NH3)2+(aq) Ag(NH3)2+(aq) is a complex ion; NH3 is a donor atom; Ag+ is a ligand Ag(NH3)2+(aq) is an acceptor ion; NH3 is a ligand; Ag+ is a complex ion Ag(NH3)2+(aq) is a complex ion; NH3 is a ligand; Ag+ is...