Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb 2 + and Fe 2 + and 0.30 M in HCl. After the solution has come to equilibrium it is saturated with H 2 S ( H 2 S [ H 2 S ] = 0.10 M ). What concentrations of Pb 2 + and Fe 2 + remain in the solution? For a saturated solution of H 2 S we can use the equilibrium: H 2 S ( a q ) + 2 H 2 O ( l ) ⇌ 2 H 3 O + ( a q ) + S 2 − ( a q ) K = 1.0 × 10 − 26 (Hint: The [H 3 O + ] changes as metal sulfides precipitate.)
Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb 2 + and Fe 2 + and 0.30 M in HCl. After the solution has come to equilibrium it is saturated with H 2 S ( H 2 S [ H 2 S ] = 0.10 M ). What concentrations of Pb 2 + and Fe 2 + remain in the solution? For a saturated solution of H 2 S we can use the equilibrium: H 2 S ( a q ) + 2 H 2 O ( l ) ⇌ 2 H 3 O + ( a q ) + S 2 − ( a q ) K = 1.0 × 10 − 26 (Hint: The [H 3 O + ] changes as metal sulfides precipitate.)
Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb2+ and Fe2+ and 0.30 M in HCl. After the solution has come to equilibrium it is saturated with H2S (
H
2
S
[
H
2
S
]
=
0.10
M). What concentrations of Pb2+ and Fe2+ remain in the solution? For a saturated solution of H2S we can use the equilibrium:
H
2
S
(
a
q
)
+
2
H
2
O
(
l
)
⇌
2
H
3
O
+
(
a
q
)
+
S
2
−
(
a
q
)
K
=
1.0
×
10
−
26
(Hint: The [H3O+] changes as metal sulfides precipitate.)
Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb2+ and Fe2+ and 0.30 M in HCl. After the solution has come to equilibrium it is saturated with H2S ([H2S] = 0.10 M). What concentrations of Pb2+ and Fe2+remain in the solution? For a saturated solution of H2S we can use the equilibrium:H2S(aq) + 2H2O(l) ⇌ 2H3O+(aq) + S2−(aq) K = 1.0 × 10−26
1) The equation below represents the equilibrium process of a saturated solution of Ca(OH)2 If the following changes are made to a saturated solution, what will be the effect on the [Ca2+]?
Ca(OH)2 (s) <--> Ca2+(aq) + 2 OH- (aq) ΔH = -16.6 kJ
A strong base is added to the solution (Decrease, Increase, No change)
More solid Ca(OH)2 is added to the container (Decrease, Increase, No change)
The solution is raised to a higher temperature (Decrease, Increase, No change)
A strong acid is added to the solution (Decrease, Increase, No change)
Ca(NO3)2 (s) is added. Ca(NO3)2 is very soluble (Decrease, Increase, No change)
6. Which of the following processes will increase the pH of a buffer solution prepared by mixing 0.89 mol
HCOOH (formic acid) and 0.76 mol HCOONa (sodium formate) into a 1-L solution? Ka (HCOOH) = 1.8 x 104.
%3D
a) add some NaCl into the buffer solution.
b) add some HCl into the buffer solution.
c) add some NaOH into the buffer solution.
d) add more water into the buffer solution.
e) None of the above.
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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