22. What will be the concentration of Ni in a solution that is made at 25°C...
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?
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?
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 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
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 formation constant of Ni(NH3)62+ is 5.5x108. 1st attempt Part 1 (1 point) What is the initial concentration of Ni(NO3), in the solution? M 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 0.500 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?
Calculate the Ni+2 concentration of a solution made by mixing 0.020 mole of solid Ni(NO3)2 into 1.0 liter of 0.22 M NH4OH. Kdfor Ni(NH3)4 2+ = 1.1 X 10^-8
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
i just want to know if i need to divide the concentration for Ni(NO3)2 in half because the molar ratio isnt 1:1. i dont need this problem to be solved. 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) K for [Ni(NH3).)?* = 2.0 x 108
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.