Ch (Net Ionic Equations)

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Ch (Net Ionic Equations)

Presentation transcript:

Ch. 11.3 (Net Ionic Equations) Many reactions take place in aqueous solutions and involve ions.

The formation of an insoluble solid (a precipitate) drives a chemical reaction. Chemists use 3 types of equations to represent aqueous ionic reactions.

Molecular, Total Ionic, and Net Ionic Equations a) Molecular Equations-complete formulas are written for all the reactants and products, no ions are written. b)Complete Ionic equations-all soluble ionic substances are written in their dissociated (ionized) forms.

c) Net Ionic equations-only those particles which are involved in a chemical reaction. All spectator ions are removed Spectator ions-those ions which do not participate in the chemical reaction but are present in the reaction mixture.

Write the molecular, complete ionic, and net ionic equations for the reaction of an aqueous solution of calcium chloride and an aqueous solution of sodium carbonate.

the molecular equation is: CaCl2(aq) + Na2CO3(aq) CaCO3(s)+2NaCl(aq) 2) the complete ionic equation is: Ca2+(aq) + 2 Cl-(aq) + 2 Na+(aq) + CO32-(aq)  CaCO3(s) + 2 Na+(aq) + 2 Cl-(aq) 3) the net ionic equation is: Ca2+(aq) + CO32- (aq)  CaCO3(s)

Predict the products when solutions of silver nitrate and sodium chromate are mixed.

PREDICTING PRECIPITATION REACTIONS USING SOLUBILITY RULES You need to know whether the predicted products are soluble or insoluble in water. Pg. 344 -Rules

Example: If we add a solution of potassium chloride to a silver nitrate solution will a precipitate form? Write the molecular, complete ionic and net ionic equations.

If we add a solution of sodium nitrate to an ammonium chloride solution will a precipitate form?