How is the molar solubility affected by addition of lead(II) nitrate to the solu
ID: 908658 • Letter: H
Question
How is the molar solubility affected by addition of lead(II) nitrate to the solution?
Molar solubility = moles of salt that dissolve per L of solution.
Hint: Consider Le Chatelier’s Principle, you are adding Pb2+ ions.
PbI2(s)DPb2+(aq) + 2I-(aq)
Decreases molar solubility, equilibrium is shifted to the left.
Increases molar solubility, equilibrium is shifted to the right.
No change, equilibrium can never be altered!
Decreases molar solubility, equilibrium is shifted to the left.
Increases molar solubility, equilibrium is shifted to the right.
No change, equilibrium can never be altered!
Explanation / Answer
The Pb2+ ions dissociated from lead iodide are already present (common to) in the mixture. Thus, the addition of Pb2+ ions from lead nitrate places stress on the previously established equilibrium.
And according to Le Châtelier's principle - the additional stress on the product side of the equilibrium results in the shift of equilibrium towards the reactants side to neutralise the effect. (From literature)
this will Decrease molar solubility, and equilibrium will shift to the left. (common ion effect)
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