The complex ion Cu(NH3)42+ is formed in a solution made of 0.0300 M Cu(NO3)2 and 0.400 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 x 1013
Suppose you have a solution that contains 0.0440 M Ca2+ and 0.0980 M Ag+. If solid Na3PO4 is added to this mixture, which of the following phosphate species would precipitate out of solution first?
When the second cation just starts to precipitate, what percentage of the first cation remains in solution?
Cu(NH3)4]2+↔Cu2+ +4NH3
ICE table
[Cu2+] |
[NH3] |
Cu(NH3)4]2+ |
||||||
initial |
0.0300M |
0.400M |
0 |
|||||
Amount reacted |
0.03-0.0300 |
0.4-4*0.0300 |
+0.0300 |
|||||
0 |
0.28 |
0.0300 |
||||||
change |
+x |
+4x |
-x |
|||||
equilibrium |
x |
0.28+4x |
0.03-x |
|||||
Kf=[ Cu(NH3)42+]/[Cu2+][NH3]^4=1.7*10^13
1/kf=[Cu2+][NH3]^4/[ Cu(NH3)42+]
Or, 1/1.7*10^13=x*(0.28+4x)^4/(0.03-x)[ignore x as x<<<0.028,0.03)
Or,0.59*10^-13=x*(0.28)^4/0.03
Or, 0.59*10^-13=x*(0.204)
Or,x=2.89*10^-13M
X=[Cu2+]=2.89*10^-13M
[NH3]=0.28+4x=0.12+4(2.89*10^-13M)=0.28M
Cu(NH3)4]2+=0.03-x=0.03- 2.89*10^-13M=0.03M
The complex ion Cu(NH3)42+ is formed in a solution made of 0.0300 M Cu(NO3)2 and 0.400 M NH3
The complex ion Cu(NH3)42+ is formed in a solution made of 0.0100 M Cu(NO3)2 and 0.300 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
A solution contains 0.0460 M Ca2+ and 0.0970 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? Ca3(PO4)2 Ag3PO4 Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution? percentage: _______ %
Suppose you have a solution that contains 0.0480 M Ca2 and 0.0910 M Ag . If solid Na3PO4 is added to this mixture, which of the following phosphate species would precipitate out of solution first? When the second cation just starts to precipitate, what percentage of the first cation remains in solution? Na3PO4?or Ag3PO4? or Ca3(PO4)2? When the second cation just starts to precipitate, what percentage of the first cation remains in solution?
Suppose you have a solution that contains 0.0470 M Ca2 and 0.0910 M Ag . If solid Na3PO4 is added to this mixture, which of the following phosphate species would precipitate out of solution first? Ca3(PO4)2 is the answer to part 1. When the second cation just starts to precipitate, what percentage of the first cation remains in solution?
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