A solution is formed by mixing 50.0 mL of 10.0 M NaX with 50.0 mL of 2.0 × 10 −3 M CuNO 3 . Assume that Cu + forms complex ions with X − as follows: Cu + ( a q ) + X − ( a q ) ⇌ C u X ( a q ) K 1 = 1.0 × 10 2 CuX ( a q ) + X − ( a q ) ⇌ C u X 2 − ( a q ) K 2 = 1.0 × 10 4 CuX 2 − ( a q ) + X − ( a q ) ⇌ C u X 3 2 − ( a q ) K 3 = 1.0 × 10 3 with an overall reaction Cu + ( a q ) + 3 X − ( a q ) ⇌ C u X 3 2 − ( a q ) K = 1.0 × 10 9 Calculate the following concentrations at equilibrium. a. Cux 3 2− b. CuX 2 − c. Cu +
A solution is formed by mixing 50.0 mL of 10.0 M NaX with 50.0 mL of 2.0 × 10 −3 M CuNO 3 . Assume that Cu + forms complex ions with X − as follows: Cu + ( a q ) + X − ( a q ) ⇌ C u X ( a q ) K 1 = 1.0 × 10 2 CuX ( a q ) + X − ( a q ) ⇌ C u X 2 − ( a q ) K 2 = 1.0 × 10 4 CuX 2 − ( a q ) + X − ( a q ) ⇌ C u X 3 2 − ( a q ) K 3 = 1.0 × 10 3 with an overall reaction Cu + ( a q ) + 3 X − ( a q ) ⇌ C u X 3 2 − ( a q ) K = 1.0 × 10 9 Calculate the following concentrations at equilibrium. a. Cux 3 2− b. CuX 2 − c. Cu +
A solution is formed by mixing 50.0 mL of 10.0 M NaX with 50.0 mL of 2.0 × 10−3M CuNO3. Assume that Cu+ forms complex ions with X− as follows:
Cu
+
(
a
q
)
+
X
−
(
a
q
)
⇌
C
u
X
(
a
q
)
K
1
=
1.0
×
10
2
CuX
(
a
q
)
+
X
−
(
a
q
)
⇌
C
u
X
2
−
(
a
q
)
K
2
=
1.0
×
10
4
CuX
2
−
(
a
q
)
+
X
−
(
a
q
)
⇌
C
u
X
3
2
−
(
a
q
)
K
3
=
1.0
×
10
3
with an overall reaction
Cu
+
(
a
q
)
+
3
X
−
(
a
q
)
⇌
C
u
X
3
2
−
(
a
q
)
K
=
1.0
×
10
9
Calculate the following concentrations at equilibrium.
What are the equilibrium concentrations when 0.25 mol Ni2+ is added to 1.00 L of 2.00 M NH3 solution? Ni2+(aq) + 6NH3(aq) ⇌ Ni(NH3)6 2+(aq) Kc = 5.5 × 108With such a large equilibrium constant, first form as much product as possible, then assume that only a small amount (x) of the product shifts left. Calculate the error in your assumption.
•
A mixture is prepared by combining 3.0 mL of 0.0050 M NaSCN (in 0.10 M HNO3) solution with 4.0
mL of 0.0030 M Fe(NO3)3 solution, and 3.0 mL of 0.10 M HNO3 solution.
Based on your average Kf value, determine the equilibrium concentrations
of Fe 3+, SCN, and FeSCN2+ in the solution. You cannot apply a small x approximation.
A chemistry graduate student is given 100.mL of a 0.40M trimethylamine ((CH3)3N) solution. Trimethylamine is a weak base with =Kb×7.410−4. What mass of (CH3)3NHCl should the student dissolve in the (CH3)3N solution to turn it into a buffer with pH =10.35? You may assume that the volume of the solution doesn't change when the (CH3)3NHCl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell