Chemical Equilibria Worksheet Page 2
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1
2Chemist’s Daily
Chapter 16 - Ksp
1. Exactly 200 mL of a 0.0040 BaCl
solution are added to exactly 600 mL of 0.0080 M
2
K
SO
. Will a precipitate form?
2
4
Solubility rules tell us the only possible precipitate is barium sulfate, so we need only
concern ourselves with the initial concentrations of Ba
2+
and SO
2-
. We are diluting
4
both solutions, so we must calculate the new initial concentrations:
200 mL (0.0040 M Ba
2+
) = 800 mL (? M Ba
2 +
)
[Ba
2+
] = 0.0010 M
600 mL (0.0080 M SO
2-
) = 800 mL (? M SO
2-
)
4
4
[SO
2-
] = 0.0060 M
4
The ion product is [Ba
2+
] [SO
2-
] = (0.0010) (0.0060) = 6.0 x 10
-6
. Comparing this to
4
the Ksp for barium sulfate, 1.1 x 10
-10
, we find it to be larger than the Ksp so a
precipitate will form.
2. What is the solubility of silver chloride in a 6.5 x 10
-3
M silver nitrate solution?
Express your answer in g/L.
AgCl
Ag
+
+
Cl
-
Initial
6.5 x 10
-3
M
End
6.5 x 10
-3
M
x M
Ksp = [Ag
+
] [Cl
-
]
1.8 x 10
-10
=
(6.5 x 10
-3
) (x)
x = 2.8 x 10
-8
solubility = (2.8 x 10
-8
mol L
-1
) (143.323 g mol
-1
) = 4.0 x 10
-6
g/L
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