Precipitation Reactions - 4 BaSO 4 HgSO 4 CaSO 4 and AgSO 4...

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Precipitation Reactions Precipitate  - an insoluble solid formed by a reaction in solution. Consider the following molecular equation: AgNO 3 (aq)  + NaCl (aq)    AgCl (s)  + NaNO 3 (aq) The net ionic equation of the above molecular equation is: Ag + (aq)  + Cl - (aq)    AgCl (s) In order to know which ions will combine to form precipitates, we have the  solubility  rules Solubility Rules 1. All salts containing NH 4 +  and group IA cations (Li + , Na + , K + , Rb + , Cs + , )  are  soluble . 2. All salts containing NO 3 - , C 2 H 3 O 2 - , HClO 3 - , and ClO 4 -  are  soluble . 3. All salts containing Cl - , Br - , and I -  are  soluble , except those with Ag + , Hg 2 2+ and Pb 2+ 4. All salts containing SO 4 2-  are  soluble , except PbSO
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Unformatted text preview: 4 , BaSO 4 , HgSO 4 , CaSO 4 , and AgSO 4 . 5. Most salts containing O 2-, OH-, PO 4 3-, CO 3 2-, and S 2- are insoluble , except those containingNH 4 + and group IA cations. Determine the net ionic equation for the following reaction: Ba(NO 3 ) 2 + Na 2 SO 4 → BaSO 4 + 2NaNO 3 Rule number 4 tells us that BaSO 4 is insoluble. So we can write the complete ionic equation as Ba 2+ (aq) +2 NO 3-(aq) +2 Na + (aq) +SO 4 2-(aq) → BaSO 4 (s) +2 Na + (aq) +NO 3-(aq) Removing the spectator ions leaves us with the net ionic equation: Ba 2+ (aq) + SO 4 2-(aq) → BaSO 4 (s)...
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Precipitation Reactions - 4 BaSO 4 HgSO 4 CaSO 4 and AgSO 4...

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