Question
In: Chemistry
One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution that is 0.400 M in...
One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution
that is 0.400 M in ammonia.
The formation constant of Ni(NH3)62+ is 5.5×10^8.
What is the equilibrium concentration of Ni2+(aq ) in
the solution?
Solutions
Expert Solution
Ni^2+(aq) + 6 NH3(aq) <---> Ni(NH3)6^2+(aq)
initial 1/260 = 0.00385 M 0.4 M 0 M
change x M 6x M x M
equilibrium 0.00385-x 0.4-6x x
Kf = [Ni(NH3)6^2+]/[Ni^2+][NH3]^6
at equilibrium, [NH3] = 0.4-6X = 0.4 M
(5.5*10^8) = x/((0.00385-x)(0.4)^6)
x = 0.0038499
at equilibrium, [Ni^2+] = 0.00385-0.0038499 = 1*10^-7 M
queen_honey_blossom answered 2 years agoRelated Solutions
One millimole of Ni(NO3)2 dissolves in 210.0 mL of a solution that is 0.500 M in...
One millimole of Ni(NO3)2 dissolves in 210.0 mL of a solution
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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 210mL of a solution that is .500M in NH3. (a)...
One millimole of Ni(NO3)2 dissolves in 210mL of a solution that
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(a) What is the initial concentration of Ni(NO3)2 in the
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------> The answer to (a) is .00476 M. I just can't figure
out part (b)
(b) What is the equilibrium concentration of Ni^2+(aq) in the
solution?
HINT: The Ni^2+ forms a hexammonia complex: Ni(NH3)6^2+. Kf =
5.5 x 10^8.
Please answer both questions. One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that...
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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.
1. What is the initial concentration of
Ni(NO3)2 in the solution?
2. What is the equilibrium concentration of
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