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How do the concentrations of $\mathrm{Pb}^{2+}$ and $\mathrm{S}^{2-}$ change when $\mathrm{K}_{2} \mathrm{S}$ is added to a saturated solution of PbS?
concentration of $\mathrm{Pb}^{2+}$ and $\mathrm{S}^{2-}$ ions decreases when $\mathrm{K}_{2} \mathrm{S}$ is added to a saturated solution of $\mathrm{PbS}$ .
Chemistry 102
Chapter 15
Equilibria of Other Reaction Classes
Chemical Equilibrium
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So here I have a saturated solution of, um led to sulfide and that means that I'm at equilibrium. And so the lead ion and sulphide ion concentrations are not going to change unless something happens. So we add que tu es initially were increasing the concentration of sulphide ion Know what that's gonna do with this equilibrium system with the lead sulfide? You look, it lists at leas principle by increase the concentration of sulfide. The reaction is going to switch to the direction that relieves that stress or relieves, or, in this case, removes the extra sulphide to get to it's original concentration. So the concentration of sulphide with respect to the lead sulphide equilibrium is going to decrease because now I have too much in solution and the reaction is going to move to the left towards the production of the solid lead sulphide. So the concentration and since it's moving in this direction, not only is the concentration of sulphide gonna go down, the concentration of lead would also go down because we're producing the solid lead sulphide in the beaker
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