The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is
a generic metal. A...
The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is
a generic metal. A 0.140-mole quantity of M(NO3)2 is added to a
liter of 0.890 M NaCN solution. What is the concentration of M2
ions at equilibrium?
The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is
a generic metal. A 0.140-mole quantity of M(NO3)2 is added to a
liter of 0.890 M NaCN solution. What is the concentration of M +2
ions at equilibrium?
The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is
a generic metal. A 0.170-mole quantity of M(NO3) is added to a
liter of 0.570 M NaCN solution. What is the concentration of M ions
at equilibrium?
The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is
a generic metal.
A 0.160-mole quantity of M(NO3) is added to a liter of 0.720 M
NaCN solution. What is the concentration of M ions at
equilibrium?
The formation constant* of [M(CN)6]4– is 2.50 × 1017, where M is
a generic metal.
A 0.160-mole quantity of M(NO3)2 is added to a liter of 1.460 M
NaCN solution.
What is the concentration of M2 ions at equilibrium?
Please post all of your work with it! I have tried 3 seperate
times and have gotten the wrong answer each time. The first and
third time I got 1.00 x 10^-20 and the second I got 4.00 x
10^-20.
The formation constant* of [M(CN)6]4– is 2.50 × 1017, where M is
a generic metal. A 0.130-mole quantity of M(NO3)2 is added to a
liter of 1.150 M NaCN solution. What is the concentration of M2
ions at equilibrium?
The formation constant* of [M(CN)6]4– is 2.50 × 10^17, where M
is a generic metal. A 0.160-mole quantity of M(NO3)2 is added to a
liter of 1.230 M NaCN solution. What is the concentration of M2
ions at equilibrium?
Consider an amphoteric hydroxide, M(OH)2(s), where M is a
generic metal. M(0H)2 yields M+2OH M(OH)2 +2OH yields (M(OH4)2-
Ksp=3x10^-16 Kf= .05 Estimate the solubility of M(OH)2 in a
solution buffered at pH = 7.0, 10.0, and 14.0.
At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2
, is mixed with pure water. The resulting equilibrium solution has
a pH of 10.34 . What is the ?sp of the salt at 22 °C?
A solution contains 0.25 M Pb2+ and 0.44 M Al3+. Calculate the
pH range that would allow Al(OH)3 to precipitate but not Pb(OH)2.
The Ksp values for Al(OH)3 and Pb(OH)2 can be found in this
table.
Choose the most likely pattern for the crystal field diagram for
the complex
trans–[Ni(NH3)2(CN)4]2–
where CN– produces a much stronger crystal field than
does NH3.?
From the answer the pattern show it is a square planer. Could
anyone explain it? why is not octahedral?
Consider an ionic compound, MX2 , composed of generic metal M
and generic, gaseous halogen X . The enthalpy of formation of MX2
is Δ?∘f=−677 kJ/mol. The enthalpy of sublimation of M is Δ?sub=161
kJ/mol. The first and second ionization energies of M are IE1=647
kJ/mol and IE2=1377 kJ/mol. The electron affinity of X is Δ?EA=−339
kJ/mol. (Refer to the hint). The bond energy of X2 is BE=221
kJ/mol. Determine the lattice energy of MX2 . Δ?lattice= kJ/mol