As the above hopefully shows, the common ion effect is governed by Le Chatelier’s principle.This would produce more OH - ions to rebalance those that were lost when Pb(OH) 2 (s) started forming. The same could be done with the OH - ions dissolved adding Pb(NO 3) 2 to the solution would cause Pb(OH) 2 (s) to precipitate and the equilibrium will shift to the right. Remember that Na like NO 3 - \, is a spectator ion and will not form a precipitate! The Ca(OH) 2 equilibrium will respond by shifting to the right to produce more Ca 2 ions. If we added sodium carbonate, Na 2CO 3, we would begin to precipitate CaCO 3 (s) while reducing the Ca 2 (aq) concentration. Using a solubility table, we can see that compounds containing sodium ions (Na ) will dissolve in water, and that calcium carbonate, CaCO 3, has low solubility. To do this, we need to add a compound that will reduce the amount of Ca 2 or OH - ions in solution by precipitating one of the ions out of solution.
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