The dissolution of lead (II) chloride is shown by the equilibrium equation 2PbCl

Question

The dissolution of lead (II) chloride is shown by the equilibrium equation

2PbCl2 --> Pb (2+) + 2Cl-

Which of the following statements concerning this reaction is not correct?

By Le Chateliers principle if you add more Cl- you will cause the precipitation of more PbCl2, By placing the PbCl2 in an aqueous solution that contains 0.1 M of HCl, a strong acid you directly affect the solubility constant of the PbCl2, Introducing more PbCl2 will cause the equilibrium to shift to the left, or By Le Chateliers principle, if you add more Pb (2+) you will also cause the precipitation of more PbCl2

Explanation / Answer

1) By Le Chateliers principle if you add more Cl- you will cause the precipitation of more PbCl2:

correct : on addition of Cl- the equilibrium will shift towards backward direction and hence will cause precipitation of PBCl2

2) By placing the PbCl2 in an aqueous solution that contains 0.1 M of HCl, a strong acid you directly affect the solubility constant of the PbCl2: Correct

On addition of HCl we are adding more of common ion (Cl-) so the reaction will shift to nullify the effect
( hence will shift backwards), hence the solubility of PbCl2 will decrease

3) Introducing more PbCl2 will cause the equilibrium to shift to the left.: Incorrect

If we will add PbCl2 the reaction will shift so that the effect is nullified, hence the reaciton will move forward direction to give more of Pb+2 and Cl-, hence the solubility will increase

4) if you add more Pb (2+) you will also cause the precipitation of more PbCl2 : Correct

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