A solution is prepared in which 0.00100 mol of Ni(NO3)2 and
0.500 mole of NH3 are...
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?
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?
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.
The complex ion Cu(NH3)42 is formed in a solution made of 0.0400
M Cu(NO3)2 and 0.500 M NH3. What are the concentrations of Cu2 ,
NH3, and Cu(NH3)42 at equilibrium? The formation constant*, Kf, of
Cu(NH3)42 is 1.70 × 1013.
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?
100.0 mL of 0.500 M lead(II) nitrate (Pb(NO3)2, 331
g/mol) and 100.0 mL of 0.500 M sodium sulfate (Na2SO4, 142 g/mol)
are mixed together.
(I) Write the overall balanced equation. Include the
states of each species.
(II) Write the overall (or total) ionic equation for the
reaction. Identify any spectator ions. Include states of each
species.
(III) Write the net ionic equation. Include states of
each species.
(IV) Determine the limiting reactant and the theoretical
yield of the non-aqueous product....
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?
(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. Calculate the concentrations of K1 and NO3 2 in an aqueous
solution prepared by dissolving 30.3 g KNO3 in enough water to make
300. mL of solution.
B. Calculate the concentrations of Al13 and SO4 22 in an aqueous
solution prepared by dissolving 17.1 g Al2 (SO4 ) 3 in enough water
to make 400. mL of solution.
C. Calculate the concentrations of Na1 and SO4 22 in an aqueous
solution prepared by dissolving 852 g Na2 SO4 in...
a buffer solution is prepared by mixing 100cm3 aqueous NH3 0.1mol
dm-3 with 100cm3 NH4Cl mol dm-3 . Given that KB for NH3
=1.74x10^-5
...
1) calculate pH of the buffer solution.
...
2)calculate the solution after addition 50cm3 HCl of 0.1 mol
dm-3.
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?