Complete and balance the precipitation reactions. include physical states. refer to the solubility rules as necessary. precipitation reaction: ba(no3)2(aq)+cuso4(aq)⟶baso4+cu(no3 )2 ba ( no 3 ) 2 ( aq ) + cuso 4 ( aq ) ⟶ baso 4 + cu ( no 3 ) 2 precipitation reaction: k3po4(aq)+mgcl2(aq)⟶6kcl(aq)+mg3(po 4)2(s) k 3 po 4 ( aq ) + mgcl 2 ( aq ) ⟶ 6 kcl ( aq ) + mg 3 ( po 4 ) 2 ( s )

Ba(NO₃)₂(aq) + CuSO₄(aq) ⟶ BaSO₄(s) + CU(NO₃)₂(aq)

2K₃PO₄(aq) + 3MgCl₂(aq) ⟶ 6KCl(aq) + Mg₃(PO₄)₂(s)

Ba(NO₃)₂(aq) + CuSO₄(aq) ⟶ BaSO₄(s) + CU(NO₃)₂(aq)

2K₃PO₄(aq) + 3MgCl₂(aq) ⟶ 6KCl(aq) + Mg₃(PO₄)₂(s)

A precipitation reaction is a reaction in which a mixture of aqueous reactants yields an insoluble product.

Aqueous solutions contains species that are soluble in water. Sometimes, a mixture of aqueous reactants yields a product that is insoluble in water. Such a product is called a precipitate and the reaction is a precipitation reaction.

The following are examples of balanced precipitation reactions;

In the first reaction, the precipitate formed is BaSO4 while in the second reaction, the precipitate formed is Mg3(PO4)2. According to the solubility rules, sulfates and phosphates of group 2 cations are insoluble in water.

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  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-