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Predicting Precipitation Reactions

Example on Predicting Precipitation Reactions

Predict the result of mixing reasonably concentrated solutions of the following ionic compounds. If precipitation is expected, write a balanced net ionic equation for the reaction.

(a) potassium sulfate and barium nitrate
(b) lithium chloride and silver acetate
(c) lead nitrate and ammonium carbonate

Solution

(a) The two possible products for this combination are KNO3 and BaSO4. The solubility guidelines indicate BaSO4 is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is

\(\mathrm{Ba^{2+}}(aq) + \mathrm{SO_4^{2−}}(aq) \longrightarrow \mathrm{BaSO_4}(s)\)

(b) The two possible products for this combination are LiC2H3O2 and AgCl. The solubility guidelines indicate AgCl is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is

\(\mathrm{Ag^{+}}(aq) + \mathrm{Cl^{−}}(aq) \longrightarrow \mathrm{AgCl}(s)\)

(c) The two possible products for this combination are PbCO3 and NH4NO3. The solubility guidelines indicate PbCO3 is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is

\(\mathrm{Pb^{2+}}(aq) + \mathrm{CO_3^{2−}}(aq) \longrightarrow \mathrm{PbCO_3}(s)\)

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