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 +
Solution Summary: The author explains that the equilibrium constant expression is expressed by the formula, K=Concentration
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.
A solution contains 10-28 M TOTCO3 and is at pH 8.1. How much HCI (moles per liter of
solution) is required to titrate the solution to pH 7.0? (H2CO3: pKa1=6.35, pKa2=10.33)
Don't used Ai solution
The standard Gibbs energies of formation of CaO(s), CaCO3 (calcite), and CO2 (g) are
-604.04, -1128.80, and -394.37 kJ/mol, respectively. Find the value of AG, and Keq for the
following reaction:
CaCO3 CaO (s) + CO2 (g)
[ap
A dry mixture containing 1 g of each solid [CaCO3(s) and CaO(s)] is on the lab bench in
contact with the atmosphere, which contains a partial pressure of 10-35 bar CO2 (g). What is
the total Gibbs free energy of the system containing all three species before any reaction has
happened? Does the equilibrium driving force favor conversion of one of the solids into the
other, or are the solids equilibrated with one another?
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