write the balanced complete ionic and net ionic equations for...


write the balanced complete ionic and net ionic equations for K2SO4(aq)+BaCl2(aq)-->KCl(aq)+BaSO4(s), Al(NO3)3(aq)+NaOH(aq)-->Al(OH)3(s)+NaNO3(aq), CaCl2(aq)Na2CO3(aq)-->NaCl(aq)+CaCO3(s Na2S(aq)+Pb(C2H3O2)2(aq)-->PbS(s)+NaC2H3O2(aq)

Net Ionic Reactions

Here we are given four unbalanced precipitation reactions. We know they are precipitation reactions because the reactants are dissolved in aqueous solution (as indicated by the (aq) beside the reactants) and one of the products is solid. These reactions, once balanced, are called the molecular reaction because the reactants and products are all shown as molecules. In an ionic reaction, the compounds that are designated as aqueous in the molecular reaction are shown as separated anions and cations because when an ionic compound is dissolved in water, the ions separate from each other and diffuse freely. The solid compounds are still shown as solid, because the ions are not separated from each other. The difference between the complete and net ionic reactions is that in the compete ionic reaction, all the ions and solids are shown. In the net ionic reaction, only the cation and anions that make up the precipitate are shown on the reactant side and the solid is shown on the product side.

Answer and Explanation: 1

For each reaction, we will first balance the molecular reaction, then show the complete ionic reaction and then remove spectator ions (the ones the same on both sides of the arrow ) to get the net ionic reaction:

{eq}Balanced \:molecular\:equation:\\ K_2SO_4(aq)+BaCl_2(aq) \rightarrow 2KCl(aq)+BaSO_4(s)\\ Complete\:ionic\:reaction:\\ 2K^+(aq)+SO_4^{2-}(aq)+Ba^{2+}(aq)+ 2Cl^-(aq) \rightarrow 2K^+(aq)+ 2Cl^-(aq)+BaSO_4(s)\\ Net\:ionic\:reaction:\\ SO_4^{2-}(aq)+Ba^{2+}(aq) \rightarrow BaSO_4(s)\\ {/eq}

{eq}Balanced \:molecular\:equation:\\ Al(NO_3)_3(aq)+3NaOH(aq) \rightarrow Al(OH)_3(s)+3NaNO_3(aq)\\ Complete\:ionic\:reaction:\\ Al^{3+}(aq)+3NO_3^-(aq)+3Na^+(aq) +3OH^-(aq) \rightarrow Al(OH)_3(s)+3Na^+(aq) +3NO_3^-(aq)\\ Net\:ionic\:reaction:\\ Al^{3+}(aq) +3OH^-(aq) \rightarrow Al(OH)_3(s)\\ {/eq}

{eq}Balanced \:molecular\:equation:\\ CaCl_2(aq) + Na_2CO_3(aq) \rightarrow 2NaCl(aq)+CaCO_3(s)\\ Complete\:ionic\:reaction:\\ Ca^{2+}(aq)+2Cl^-(aq) + 2Na^+ + CO_3^{2-}(aq) \rightarrow 2Na^+ +Cl^-(aq)+CaCO_3(s)\\ Net\:ionic\:reaction:\\ Ca^{2+}(aq)+ CO_3^{2-}(aq) \rightarrow CaCO_3(s)\\ {/eq}

{eq}Balanced \:molecular\:equation:\\ Na_2S(aq)+Pb(C_2H_3O_2)_2(aq) \rightarrow PbS(s)+2NaC_2H_3O_2(aq)\\ Complete\:ionic\:reaction:\\ 2Na^+(aq)+S^{2-}(aq)+Pb^{2+}(aq)+2C_2H_3O_2^-(aq) \rightarrow PbS(s)+2Na^+(aq) +2C_2H_3O_2^-(aq)\\ Net\:ionic\:reaction:\\ S^{2-}(aq)+Pb^{2+}(aq) \rightarrow PbS(s)\\ {/eq}

Learn more about this topic:

Precipitation Reactions: Predicting Precipitates and Net Ionic Equations


Chapter 10 / Lesson 9

Study precipitate reactions. Determine precipitate solubility according to solubility rules. Learn to write ionic equations by following a molecular reaction.

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