PbI2 is only very slightly soluble in water, so the following equilibrium occurs:
PbI2(s) <=> Pb2+(aq) + 2 I-(aq)
KI and KNO3 are very soluble in water and are both fully ionized.
KI(s) => K+(aq) + I-(aq)
KNO3(s) => K+(aq) + NO3-(aq)
For 0.01 M KI solution, I- is the common ion with PbI2. The extra I- in solution causes the
equilibrium for PbI2 to shift to the left according to Le Chatelier\'s principle. Thus less PbI2
dissolves and solubility decreases. This common ion effect outweighs the ionic strength effect
below.
For 0.01 M KNO3 solution, there are no common ions. However, the ionic strength of the
solution increases compared to water (due to the presence of K+ and NO3-), which decreases the
activity coefficients and increases the concentrations of the Pb2+ and I- ions in solution. Thus
more PbI2 dissolves and solubility increases.
Ksp = a(Pb2+) x a(I-)2
= Pb2+[Pb2+] x (I-[I-])2
where a is activity and is activity coefficient.
When ionic strength increases, decreases and concentration increases to maintain constant value
of Ksp.
Solution
PbI2 is only very slightly soluble in water, so the following equilibrium occurs:
PbI2(s) <=> Pb2+(aq) + 2 I-(aq)
KI and KNO3 are very soluble in water and are both fully ionized.
KI(s) => K+(aq) + I-(aq)
KNO3(s) => K+(aq) + NO3-(aq)
For 0.01 M KI solution, I- is the common ion with PbI2. The extra I- in solution causes the
equilibrium for PbI2 to shift to the left according to Le Chatelier\'s principle. Thus less PbI2
dissolves and solubility decreases. This common ion effect outweighs the ionic strength effect
below.
For 0.01 M KNO3 solution, there are no common ions. However, the ionic strength of the
solution increases compared to water (due to the presence of K+ and NO3-), which decreases the
activity coefficients and increases the concentrations of the Pb2+ and I- ions in solution. Thus
more PbI2 dissolves and solubility increases.
Ksp = a(Pb2+) x a(I-)2
= Pb2+[Pb2+] x (I-[I-])2
where a is activity and is activity coefficient.
When ionic strength increases, decreases and concentration increases to maintain constant value
of Ksp..
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PbI2 is only very slightly soluble in water, so the following equili.pdf
1. PbI2 is only very slightly soluble in water, so the following equilibrium occurs:
PbI2(s) <=> Pb2+(aq) + 2 I-(aq)
KI and KNO3 are very soluble in water and are both fully ionized.
KI(s) => K+(aq) + I-(aq)
KNO3(s) => K+(aq) + NO3-(aq)
For 0.01 M KI solution, I- is the common ion with PbI2. The extra I- in solution causes the
equilibrium for PbI2 to shift to the left according to Le Chatelier's principle. Thus less PbI2
dissolves and solubility decreases. This common ion effect outweighs the ionic strength effect
below.
For 0.01 M KNO3 solution, there are no common ions. However, the ionic strength of the
solution increases compared to water (due to the presence of K+ and NO3-), which decreases the
activity coefficients and increases the concentrations of the Pb2+ and I- ions in solution. Thus
more PbI2 dissolves and solubility increases.
Ksp = a(Pb2+) x a(I-)2
= Pb2+[Pb2+] x (I-[I-])2
where a is activity and is activity coefficient.
When ionic strength increases, decreases and concentration increases to maintain constant value
of Ksp.
Solution
PbI2 is only very slightly soluble in water, so the following equilibrium occurs:
PbI2(s) <=> Pb2+(aq) + 2 I-(aq)
KI and KNO3 are very soluble in water and are both fully ionized.
KI(s) => K+(aq) + I-(aq)
KNO3(s) => K+(aq) + NO3-(aq)
For 0.01 M KI solution, I- is the common ion with PbI2. The extra I- in solution causes the
equilibrium for PbI2 to shift to the left according to Le Chatelier's principle. Thus less PbI2
dissolves and solubility decreases. This common ion effect outweighs the ionic strength effect
below.
For 0.01 M KNO3 solution, there are no common ions. However, the ionic strength of the
solution increases compared to water (due to the presence of K+ and NO3-), which decreases the
activity coefficients and increases the concentrations of the Pb2+ and I- ions in solution. Thus
more PbI2 dissolves and solubility increases.
Ksp = a(Pb2+) x a(I-)2
2. = Pb2+[Pb2+] x (I-[I-])2
where a is activity and is activity coefficient.
When ionic strength increases, decreases and concentration increases to maintain constant value
of Ksp.
![PbI2 is only very slightly soluble in water, so the following equilibrium occurs:
PbI2(s) <=> Pb2+(aq) + 2 I-(aq)
KI and KNO3 are very soluble in water and are both fully ionized.
KI(s) => K+(aq) + I-(aq)
KNO3(s) => K+(aq) + NO3-(aq)
For 0.01 M KI solution, I- is the common ion with PbI2. The extra I- in solution causes the
equilibrium for PbI2 to shift to the left according to Le Chatelier's principle. Thus less PbI2
dissolves and solubility decreases. This common ion effect outweighs the ionic strength effect
below.
For 0.01 M KNO3 solution, there are no common ions. However, the ionic strength of the
solution increases compared to water (due to the presence of K+ and NO3-), which decreases the
activity coefficients and increases the concentrations of the Pb2+ and I- ions in solution. Thus
more PbI2 dissolves and solubility increases.
Ksp = a(Pb2+) x a(I-)2
= Pb2+[Pb2+] x (I-[I-])2
where a is activity and is activity coefficient.
When ionic strength increases, decreases and concentration increases to maintain constant value
of Ksp.
Solution
PbI2 is only very slightly soluble in water, so the following equilibrium occurs:
PbI2(s) <=> Pb2+(aq) + 2 I-(aq)
KI and KNO3 are very soluble in water and are both fully ionized.
KI(s) => K+(aq) + I-(aq)
KNO3(s) => K+(aq) + NO3-(aq)
For 0.01 M KI solution, I- is the common ion with PbI2. The extra I- in solution causes the
equilibrium for PbI2 to shift to the left according to Le Chatelier's principle. Thus less PbI2
dissolves and solubility decreases. This common ion effect outweighs the ionic strength effect
below.
For 0.01 M KNO3 solution, there are no common ions. However, the ionic strength of the
solution increases compared to water (due to the presence of K+ and NO3-), which decreases the
activity coefficients and increases the concentrations of the Pb2+ and I- ions in solution. Thus
more PbI2 dissolves and solubility increases.
Ksp = a(Pb2+) x a(I-)2](https://image.slidesharecdn.com/pbi2isonlyveryslightlysolubleinwatersothefollowingequili-230409132642-99b4bd76/85/pbi2-is-only-very-slightly-soluble-in-water-so-the-following-equilipdf-1-320.jpg)
![= Pb2+[Pb2+] x (I-[I-])2
where a is activity and is activity coefficient.
When ionic strength increases, decreases and concentration increases to maintain constant value
of Ksp.](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)