A 0.012-mol sample of Na2SO4 is added to 400 mL of each of two solutions. One solution contains 1.5 103 M BaCl2; the other contains 1.5 103 M CaCl2. Given that Ksp for BaSO4 = 1.5 109 and Ksp for CaSO4 = 6.1 105:
a.
BaSO4 would precipitate but CaSO4 would not.
b.
CaSO4 would precipitate but BaSO4 would not.
c.
Both BaSO4 and CaSO4 would precipitate.
d.
Neither BaSO4 nor CaSO4 would precipitate.
e.
Not enough information is given to determine if precipitation would occur.
Question 2
Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 107, 1.6 1010, and 2.0 1013, respectively. Which compound will precipitate first?
a.
CuCl
b.
AgCl
c.
AuCl
d.
All will precipitate at the same time.
e.
Cannot be determined.
Question 3
The Ksp for Mn(OH)2 is 2.0 1013. At what pH will Mn(OH)2 begin to precipitate from a solution in which the initial concentration of Mn2+ is 0.10 M?
a.
6.47
b.
13.3
c.
5.85
d.
7.03
e.
8.15
Question 4
The Ksp for BaF2 is 2.4 105. When 10 mL of 0.01 M NaF is mixed with 10 mL of 0.01 M BaNO3, will a precipitate form?
a.
No, because Q is 1 1012 and since it is less than Ksp no precipitate will form.
b.
Yes, because Q is 1 1012 and since it is less than Ksp a precipitate will form.
c.
No, because Q is 1.25 107 and since it is less than Ksp no precipitate will form.
d.
Yes, because Q is 1.25 107 and since it is less than Ksp a precipitate will form.
e.
None of the above.
pH values of common solutions
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