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![Solution Given data One millimole of Ni(nog), dissolved in 240.0ml of solution that is 0.300 m in ammonia a @ [ Ne (NO3)2] =](http://img.homeworklib.com/questions/6be98200-0f5c-11ea-8da5-d5c3c0017092.png?x-oss-process=image/resize,w_560)
![0.oouG 5,5x108 rangkat)[.000432] J : 1,75X10-8 M](http://img.homeworklib.com/questions/6c671470-0f5c-11ea-90a9-6160d4c197a8.png?x-oss-process=image/resize,w_560)
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06 Question (2 points) One millimole of Ni(NO3)2 dissolves in 240.0 mL of a solution that is 0.300 M in ammonia. The fo...
One millimole of Ni(NO3)2 dissolves in 240.0 mL of a solution that is 0.500 M in...
One millimole of Ni(NO3)2 dissolves in 240.0 mL of a solution that is 0.500 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108. What is the equilibrium concentration of Ni2+(aq ) in the solution?
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.400 M in...
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.400 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108. 1st attempt Part 1 (1 point)See HintSee Periodic Table What is the initial concentration of Ni(NO3)2 in the solution? Part 2 (1 point) What is the equilibrium concentration of Ni2+(aq ) in the solution?
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.300 M in...
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.300 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108. What is the initial concentration of Ni(NO3)2 in the solution? I already have this answer which is 4.35E-3, but I cannot figure out the second part which is: What is the equilibrium concentration of Ni2+(aq ) in the solution? and the answer IS NOT 1.08E-8
12 Question ( point) a See page 749 One millimole of Ni(NO3)2 dissolves in 260.0 mL...
12 Question ( point) a See page 749 One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution that is 0.300 M in ammonia. The formation constant of Ni(NH3)62+is 5.5x108. 5th attempt Part1 (0.5 point) Feeback Feedback see Periodic Table See Hint What is the initial concentration of Ni(NO3)2 in the solution? 0.003846M Part 2 (0.5 point) Feedback What is the equilibrium concentration of Ni2 (aq) in the solution? x 10-0 M 7.00
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.500 M in...
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.500 M in ammonia.The formation constant of Ni(NH3)62+ is 5.5×108. What is the initial concentration of Ni(NO3)2 in the solution? What is the equilibrium concentration of Ni2+(aq ) in the solution?
Please answer both questions. One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that...
Please answer both questions. One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.400 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108. What is the initial concentration of Ni(NO3)2 in the solution? What is the equilibrium concentration of Ni2+(aq ) in the solution?
helppp 12 Question (1 point) a See page 749 One millimole of Ni(NO3)2 dissolves in 230.0...
helppp
12 Question (1 point) a See page 749 One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.500 M in ammonia. The formation constant of Ni(NHa)2* is 5.5x108 6th attempt 5th attempt l See Periodic Table See Hint Part1 (0.3 point) Feedback What is the initial concentration of Ni(NO3)2 in the solution? x 10 M 4.35 Part 2 (0.5 point) Feedback What is the equilibrium concentration of Ni2 (aq) in the solution? x 10M 6.27
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...
2. You mix a 105.0 mL sample of a solution that is 0.0114 M in Ni(NO3)2...
2. You mix a 105.0 mL sample of a solution that is 0.0114 M in Ni(NO3)2 with a 190.0 mL sample of a solution that is 0.300 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+ remains? The value of Kr for [Ni(NH3)6]2+ is 2.0x108.
2. Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2. Then 10.0 mL of 0.300 M...
2. Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3).]* at equilibrium? (8 pts) Krfor [Ni(NH3).]?* = 2.0 x 108
12 Question ( point) a See page 749 One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution that is 0.300 M in ammonia. The formation constant of Ni(NH3)62+is 5.5x108. 5th attempt Part1 (0.5 point) Feeback Feedback see Periodic Table See Hint What is the initial concentration of Ni(NO3)2 in the solution? 0.003846M Part 2 (0.5 point) Feedback What is the equilibrium concentration of Ni2 (aq) in the solution? x 10-0 M 7.00
helppp
12 Question (1 point) a See page 749 One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.500 M in ammonia. The formation constant of Ni(NHa)2* is 5.5x108 6th attempt 5th attempt l See Periodic Table See Hint Part1 (0.3 point) Feedback What is the initial concentration of Ni(NO3)2 in the solution? x 10 M 4.35 Part 2 (0.5 point) Feedback What is the equilibrium concentration of Ni2 (aq) in the solution? x 10M 6.27
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...
2. You mix a 105.0 mL sample of a solution that is 0.0114 M in Ni(NO3)2 with a 190.0 mL sample of a solution that is 0.300 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+ remains? The value of Kr for [Ni(NH3)6]2+ is 2.0x108.
2. Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3).]* at equilibrium? (8 pts) Krfor [Ni(NH3).]?* = 2.0 x 108
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