Session #25: Homework Solutions
Problem #1
Bi2S3 dissolves in water according to the following reaction:
Bi2S3 (s) ⇔ 2 Bi3+ (aq) + 3 S2- (aq)
for which the solubility product, Ksp, has the value of 1.6 × 10-72 at room
temperature.
(a) At room temperature how many moles of Bi2S3 will dissolve in 3.091 × 106
liters of water?
(b) How many Bi3+ ions will be found in the solution described in part (a)?
Solution
(a)
Bi2S3 = 2 Bi3+(aq) + 3 S2- (aq)
∴ [Bi3+ ] = 2 Cs and [s2 ] = 3 Cs
∴ Ksp = (2 Cs )2 (3 Cs )3 = 4 Cs2 • 27 Cs3 = 108 Cs5
1/5
⎛ Ksp ⎞
∴ Cs = ⎜
⎜ 108 ⎟⎟
⎝
⎠
= 1.715 x 10-15 mol/L
∴ in 3.091 x 106 L ⇒ 5.3 x 10-9 mol Bi2S3
(b)
[Bi3+] = 2 Cs = 1.06 x 10–8 mol
NAv ions/mol ⇒ 6.38 x 1015 Bi3+ ions in the 3.091 x 106 liters of water of
part (a)
Problem #2
Calculate the volume of 0.25 M NaI that would be needed to precipitate all the
g2+ ion from 45 mL of a 0.10 M Hg(NO3)2 solution according to the following
reaction:
2 NaI(aq) + Hg(NO3 )2 (aq) → HgI2 (s) + 2 NaNO3 (aq)
Solution
2 NaI(aq)+Hg(NO3 )2 (aq) → HgI2 (s) + NaNO3 (aq)
0.10 mol Hg(NO3 )2
x 0.045 L = 4.5 x 10-3 mol Hg(NO3 )2
1L
4.5 x 10-3 mol Hg(NO3 )2 x
2 mol NaI
= 9.00 x 10-3 mol NaI
1 mol Hg(NO3 )2
9.00 x 10-3 mol NaI
1000ml
= 3.6 x 10-2 L x
= 36 mL NaI
mol NaI
1L
0.25
L
Problem #3
(a) Strontium fluoride, SrF2, has a Ksp value in water of 2.45 × 10–9 at room
temperature.
Calculate the solubility of SrF2 in water. Express your answer in units of
molarity.
(b) Calculate the solubility of SrF2 in 0.03 M NaF (aq). Express your answer in
units of molarity.
Assume that NaF is completely dissociated in water.
Solution
(a)
SrF2 = Sr2+ + 2 F–
Ksp = [Sr2+][F–]2 ,
but [F] = 2 [Sr2+] = 2cs
1/3
2
∴ Ksp = cs (2 cs ) = 4
(b)
cs3
∴
⎛ Ksp ⎞
cs = ⎜
⎜ 4 ⎟⎟
⎝
⎠
= 8.49 x 10-4 M
NaF = Na+ + F–
∴ [F] = 0.003 M, which dominates the other equilibrium
∴ Ksp = [Sr2+ ][F − ]2 ⇒ [Sr2+ ] =
∴ [Sr2+ ]=cs = 2.72x10−6 M
Ksp
- 2
[F ]
=
2.45x10−9
2
(0.03)
= 2.72x10−6 M
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3.091SC Introduction to Solid State Chemistry
Fall 2009
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