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Reactions in Solution

Reactions in Solution. Types of Chemical Reactions. Precipitation Reactions Acid-Base Reactions Oxidation-Reduction Reactions. Precipitation Reactions. Dissociation – Ionic compounds dissolve in water and the ions separate and move independently AgNO 3 (aq) +NaCl(aq)  products

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Reactions in Solution

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  1. Reactions in Solution

  2. Types of Chemical Reactions • Precipitation Reactions • Acid-Base Reactions • Oxidation-Reduction Reactions

  3. Precipitation Reactions • Dissociation – Ionic compounds dissolve in water and the ions separate and move independently AgNO3(aq) +NaCl(aq)  products Ag+(aq)+NO3-(aq) + Na+(aq) +Cl-(aq) products • Determination of Products • Recombination of ions – AgNO3, NaCl, AgCl, NaNO3 • Elimination of reactants as products (no AgNO3 or NaCl)

  4. Identify the precipitate • “Switch partners” • AgCl and NaNO3 are the products • AgCl is insoluble, so it is the white precipitate • If there is no insoluble product, the reaction does not occur

  5. Solubility Rules for Salts in Water • Most nitrate salts (NO3-) are soluble • Most salts contain the alkali metals (Li+, Na+,K+,Cs+,Rb+) and the ammonium (NH4+) ion are soluble. • Most chloride, bromide and iodide salts are solutble. Exceptions are salts containing the ions Ag+, Pb2+ and Hg2+. • Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, HgSO4, and CaSO4. • Most hydroxide salts are only slightly soluble. NaOH and KOH are soluble, but hydroxides of Ba, Sr and Ca are only marginally soluble. • Most sulfides (S2-), carbonate (CO32-), chromate(CrO42-)and phosphate (PO43-) salts are only slightly soluble.

  6. Molecular Equation Na2CO3(aq) + Ca(NO3)2(aq) 2NaNO3(aq) + CaCO3(s) Complete Ionic Equation 2Na+(aq)+CO32-(aq) + Ca2+(aq)+2NO3-(aq) 2Na+(aq)+ 2NO3-(aq) + CaCO3(s) Net Ionic Equation Ca2+(aq) + CO32-(aq) CaCO3(s) Describing Reactions in Solution

  7. Solubility Chart

  8. AP Reaction Questions • solid barium peroxide is added to cold dilute sulfuric acid • hydrogen sulfide gas is added to a solution of cadmium nitrate • dilute sulfuric acid is added to a solution of barium acetate • a precipitate is formed when solutions of trisodium phosphate and calcium chloride are mixed • A solution of sodium hydroxide is added to a solution of lead(II) nitrate

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