What is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2? Ksp = 6.65×10?18 for M(OH)2 Calculate the molar solubility of lead thiocyanate in 0.600 M KSCN.? Ksp=2.00* 10^-5
Both the problems are examples common ion effect.
Let x be the molar solubility of M(OH)2. The dissociation of M(OH)2 can be written as
M(OH)2 (s) <======> M2+ (aq) + 2 OH- (aq)
x x 2x
Again, the ionization of M(NO3)2 can be written as
M(NO3)2 (aq) ---------> M2+ (aq) + 2 NO3- (aq)
0.202 M 0.202 M
We do not bother about the concentration of NO3- since it doesn’t play any role in the precipitation reaction. We next set up the ICE chart as
M(OH)2 (aq) <=====> M2+ (aq) + 2 OH- (aq)
initial x 0.202 0
change - x + x + 2x
equilibrium - (0.202 + x) 2x
We need to account for the M2+ furnished by the M(NO3)2. The solubility product is
Ksp = (0.202 + x)(2x)2
Next, we make an approximation. Since the value of Ksp = 6.65*10-18 is quite low, we will expect x<<0.202 and hence, (0.202 + x) ≈ 0.202. Therefore,
Ksp = (0.202).(2x)2
===> 6.65*10-18 = 0.202*4x2
===> x2 = 8.230*10-18
===> x = 2.868*10-9
The molar solubility of M(OH)2 in 0.202 M M(NO3)2 is 2.868*10-9 M ≈ 2.9*10-9 M (ans).
We follow the same logic as before. The concentration of SCN- from KSCN is 0.600 M [1:1 dissociation as per the equation KSCN (aq) ----------> K+ (aq) + SCN- (aq)].
The ionization of lead thiocyanate, Pb(SCN)2 follows the equation
Pb(SCN)2 (s) <=====> Pb2+ (aq) + 2 SCN- (aq)
x x 2x
Ksp = (x).(2x + 0.600)2
Now, we shall again assume (2x + 0.600) ≈ 0.600; therefore,
Ksp = x.(0.600)2
===> 2.0*10-5 = x.(0.36)
===> x = 5.555*10-5
The molar solubility of Pb(SCN)2 in 0.600 M KSCN is 5.555*10-5 M ≈ 5.5*10-5 M (ans).
What is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2? Ksp = 6.65×10?18...
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Lead thiocyanate, Pb(SCN)2, has a Ksp value of 2.00×10−5. a) Calculate the molar solubility of lead thiocyanate in pure water. The molar solubility is the maximum amount of lead thiocyanate the solution can hold. b) Calculate the molar solubility of lead thiocyanate in 0.500 M KSCN.
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The generic metal hydroxide M(OH)2 has Ksp = 5.85×10−18. A. What is the solubility of M(OH)2 in pure water? B. What is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2?
What is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2?
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