What is the equilibrium concentration of Ni^2+ (aq) in the
solution. If one millimole of Ni(NO3)2...
What is the equilibrium concentration of Ni^2+ (aq) in the
solution. If one millimole of Ni(NO3)2 dissolves in 220.0 mL of a
solution that is 0.300 M in ammonia?
One millimole of Ni(NO3)2 dissolves in 210mL of a solution that
is .500M in NH3.
(a) What is the initial concentration of Ni(NO3)2 in the
solution?
------> 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.
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?
One millimole of Ni(NO3)2 dissolves in 210.0 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.
1. What is the initial concentration of
Ni(NO3)2 in the solution?
2. What is the equilibrium concentration of
Ni2+(aq ) in the solution?
Using (Kf=1.2×109) calculate the concentration of Ni2+(aq),
assuming that it is present as Ni(NH3)2+6, at equilibrium after
dissolving 1.28 gNiCl2 in 100.0 mL of 0.20 MNH3(aq).
Using the appropriate Ksp values, find the concentration of NO3−
ions in the solution at equilibrium after 700 mL of 0.35 M aqueous
Cu(NO3)2 solution has been mixed with 350 mL of 0.40 M aqueous KOH
solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19). Now find
the concentration of OH− ions in this solution at equilibrium.
(Enter in M.)
(A) A current of 4.62 A is passed through a Ni(NO3)2 solution
for 1.70 hours. How much nickel is plated out of the solution?
(B) A current of 4.09 A is passed through a Cr(NO3)2 solution.
How long (in hours) would this current have to be applied to plate
out 7.70 g of chromium?
A solution is prepared in which 0.00100 mol of Ni(NO3)2 and
0.500 mole of NH3 are dissolved in a total volume of 1.00 L. What
is the concentration of Ni(H2O)62+ ions in the solution at
equilibrium?
Calculate the equilibrium concentration of Ag+(aq ) in a
solution that is initially 0.170 M AgNO3 and 0.990 M NH3, and in
which the following reaction takes place:
Ag+(aq)+2NH3(aq)=Ag(NH3)2+(aq) (Kf = 1.70x107)
4. Calculate the equilibrium concentration of Ag+
(aq) in a solution that is initially 0.150 M AgNO3 and
0.500 M KCN. The formation constant for
[Ag(CN)2]- (aq) is Kf= 1.0 x
1021
a. 8.9 x 10-21 M
b. 2.3 x 10 -21 M
c. 4.3 x 10 -22 M
d. 7.5 x 10 -22 M
e. 3.8 x 10 -21 M
5. If a solution of Pb(NO3)2 (aq) is mixed
with a solution of NaBr(aq), what condition would cause
precipitation...