The following equation represents a saturated solution of lead chromate PbCrO4(s) ⇌ Pb2+(aq) + CrO4 2–...
The following equation represents a saturated solution of lead chromate
PbCrO4(s) ⇌ Pb2+(aq) + CrO4 2– (aq) Ksp at 298 K was determined to be 1.8 x10^–14. What will happen if solid lead nitrate is added to the system?
(A) Have no effect.
(B) Reduce the value of the Ksp for lead chromate.
(C) Increase the value of Ksp for lead chromate.
(D) Shift the reaction to the right.
(E) Shift the reaction to the left.
Homework Answers
Ksp of compound depends only on temperature.
So, Ksp will not change by changing concentration.
Pb(NO3)2 when added will give Pb2+ which is product in given equilibrium reaction of PbCrO4.
So, it is like adding more product and hence equilibrium will shift to left. This is called as common ion effect.
Answer: E
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The following equation represents a saturated solution of lead
chromate
PbCrO4(s) ⇌ Pb2+(aq) + CrO4 2–...
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Consider the dissolution equation of lead(II) chloride. PbCl2 (s) Pb2+ (aq) + 2 C1- (aq) Suppose you add 0.2331 g of PbCl2(s) to 50.0 mL of water. In the resulting saturated solution, you find that the concentration of Pb2+ (aq) is 0.0159 M and the concentration of Cl - (aq) is 0.0318 M. What is the value of the equilibrium constant, Ksp, for the dissolution of PbCl2? Answer:
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