"calculate the concentration of Ag+ present in a solution at equilibrium when concentrated ammonia is added...
"calculate the concentration of Ag+ present in a solution at equilibrium when concentrated ammonia is added to a 0.010m solution of AgNO3 to give an equilibrium concentration of (NH3)= 0.20 m. Neglect the small volume change that occurs when NH3 is added
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"calculate the concentration of Ag+ present in a solution at
equilibrium when concentrated ammonia is added...
Calculate [Ag+] at equilibrium when 0.220 M concentrated ammonia, NH3, is added to 0.020 M AgNO3....
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.
3. (4 pts) a) Decreasing the concentration of free metal ion in solution by complexing it...
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 concentration of Ag (aq) in a solution that is initially 0.140 M AgNO3...
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
Iul See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution...
Iul See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.120 M AgNO, and 0.840 MNH3, and in which the following reaction takes place: Ag (aq) + 2NH, (aq) (NH)2(aq) (K - 1.70.10) M Ag One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.500 M in ammonia The formation constant of Ni(NH3)2 is 5,5x10% 1st attempt Part 1 (1 point) i See Periodic Table See Hint...
40. Concentrated aqueous ammonia is added to a solution of copper(II) sulfate. A white precipitate forms....
40. Concentrated aqueous ammonia is added to a solution of copper(II) sulfate. A white precipitate forms. The precipitate dissolves as more ammonia is added, generating an intensely blue solution. Which combination of net ionic equations, in the appropriate order, describes this chemistry?! I Cu?* (aq) + 2OH(aq) Cu(OH)2 (19) II Cu?" (aq) + 2OH(aq) = Cu(OH)2 (8) III Cu(OH)(aq) + 4 NH, (aq) Cu(NH3),?* () + 2OH(aq) IV Cu(OH)2 (8) + 4NH, (aq) Cu(NH3)*(14) + 2OH(aq) V NH3(aq) + H20...
tl See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution...
tl See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.200 M AgNO3 and 0.650 MNH3, and in which the following reaction takes place: A a)2NH, (a)Ag(NIH)(ag (K-1.70.10) 10M Ag 2.90
A solution of Na3PO4 is added dropwise to a solution that is 0.0810 M in Ag+...
A solution of Na3PO4 is added dropwise to a solution that is 0.0810 M in Ag+ and 0.00171 M in Cu2+. The Ksp of Ag3PO4 is 8.89e-17. The Ksp of Cu3(PO4)2 is 1.4e-37. (a) What concentration of PO43- is necessary to begin precipitation? (Neglect volume changes.) [PO43-] = M. (b) Which cation precipitates first? Ag+ Cu2+ (c) What is the concentration of PO43- when the second cation begins to precipitate? [PO43-] = M.
Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.200 M AgNO3...
Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.200 M AgNO3 and 0.200 M KCN. The formation constant for [Ag(CN)2] (aq) is Ka= 1.0 x 10^21. Show your work for each step. a. 5.6 x 10^-22 M b. 5.0 X 10^-22 M c. 3.3 x 10^-33 M d. 1.0 x 10^-30 M e. 1.3 x 10^-21 M
Calculate [Cu2+] at equilibrium when 0.20 mol of CuSO4 is added to 1.000 L of 1.20...
Calculate [Cu2+] at equilibrium when 0.20 mol of CuSO4 is added to 1.000 L of 1.20 M NH3 solution. Kf for [Cu(NH3)4]2+ is 5.0 × 1013.
all 5&6 5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(a...
all 5&6
5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
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 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
Iul See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.120 M AgNO, and 0.840 MNH3, and in which the following reaction takes place: Ag (aq) + 2NH, (aq) (NH)2(aq) (K - 1.70.10) M Ag One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.500 M in ammonia The formation constant of Ni(NH3)2 is 5,5x10% 1st attempt Part 1 (1 point) i See Periodic Table See Hint...
40. Concentrated aqueous ammonia is added to a solution of copper(II) sulfate. A white precipitate forms. The precipitate dissolves as more ammonia is added, generating an intensely blue solution. Which combination of net ionic equations, in the appropriate order, describes this chemistry?! I Cu?* (aq) + 2OH(aq) Cu(OH)2 (19) II Cu?" (aq) + 2OH(aq) = Cu(OH)2 (8) III Cu(OH)(aq) + 4 NH, (aq) Cu(NH3),?* () + 2OH(aq) IV Cu(OH)2 (8) + 4NH, (aq) Cu(NH3)*(14) + 2OH(aq) V NH3(aq) + H20...
tl See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.200 M AgNO3 and 0.650 MNH3, and in which the following reaction takes place: A a)2NH, (a)Ag(NIH)(ag (K-1.70.10) 10M Ag 2.90
all 5&6
5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
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