The equilibrium constant for the following reaction is 1.0 × 10 23 : Cr 3+ ( a q ) + H 2 E D T A 2 − ( a q ) ⇌ C r E D T A − ( a q ) + 2 H + ( a q ) EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt Na 2 H 2 EDTA, are used to treat heavy metal poisoning. Calculate [Cr 3+ ] at equilibrium in a solution originally 0.0010 M in Cr 3+ and 0.050 M in H 2 EDTA 2− and buffered at pH = 6.00.
The equilibrium constant for the following reaction is 1.0 × 10 23 : Cr 3+ ( a q ) + H 2 E D T A 2 − ( a q ) ⇌ C r E D T A − ( a q ) + 2 H + ( a q ) EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt Na 2 H 2 EDTA, are used to treat heavy metal poisoning. Calculate [Cr 3+ ] at equilibrium in a solution originally 0.0010 M in Cr 3+ and 0.050 M in H 2 EDTA 2− and buffered at pH = 6.00.
Solution Summary: The author calculates the value of left[Cr+right] at equilibrium in a solution.
The equilibrium constant for the following reaction is 1.0 × 1023:
Cr
3+
(
a
q
)
+
H
2
E
D
T
A
2
−
(
a
q
)
⇌
C
r
E
D
T
A
−
(
a
q
)
+
2
H
+
(
a
q
)
EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt Na2H2EDTA, are used to treat heavy metal poisoning. Calculate [Cr3+] at equilibrium in a solution originally 0.0010 M in Cr3+ and 0.050 M in H2EDTA2− and buffered at pH = 6.00.
What is the concentration of Ag+ at equilibrium in the following reaction when carried out at 238 K and [Fe2+] = [Fe3+] = 0.3 M at equilibrium?
The blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium.
Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1)
Upon addition of LiCl to this equilibrium in solution, which observation would be expected?
The solution turns blue.
The solution turns yellow.
The Cu2+ salts precipitate out of solution.
The volume of water decreases.
Incorrect
O O O
An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L.
Kf for Ni(NH3)62+ is equal to 5.5 × 108.
Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed
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