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Precipitation reactions

Precipitation reactions. The Reaction of K 2 CrO 4 ( aq ) and Ba (NO 3 ) 2 ( aq ). Simple Rules for Solubility. Most nitrate (NO 3  ) salts are soluble. Most alkali (group 1A) salts and NH 4 + are soluble. Most Cl  , Br  , and I  salts are soluble (NOT Ag + , Pb 2 + , Hg 2 + )

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Precipitation reactions

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  1. Precipitation reactions

  2. The Reaction of K2CrO4(aq) and Ba(NO3)2(aq)

  3. Simple Rules for Solubility • Most nitrate (NO3) salts are soluble. • Most alkali (group 1A) salts and NH4+ are soluble. • Most Cl, Br, and I salts are soluble (NOT Ag+, Pb2+, Hg2+) • Most sulfate salts are soluble (NOT BaSO4, PbSO4, HgSO4, CaSO4) • Most OH salts are only slightly soluble (NaOH, KOH are soluble, Ba(OH)2, Ca(OH)2 are marginally soluble) • Most S2, CO32, CrO42, PO43 salts are only slightly soluble.

  4. Describing Reactions in Solution • Molecular equation (reactants and products as compounds) • AgNO3(aq) + NaCl(aq)AgCl(s) + NaNO3(aq) • Complete ionic equation (all strong electrolytes shown as ions) • Ag+(aq) + NO3(aq) + Na+(aq) + Cl(aq)  AgCl(s) + Na+(aq) + NO3(aq)

  5. Describing Reactions in Solution (continued) • Net ionic equation (show only components that actually react) Ag+(aq) + Cl(aq) AgCl(s) Na+ and NO3 are spectator ions.

  6. precipitate Pb(NO3)2(aq) + 2NaI (aq) PbI2(s) + 2NaNO3(aq) Pb2+ + 2NO3- + 2Na+ + 2I- PbI2 (s) + 2Na+ + 2NO3- Pb2+ + 2I- PbI2 (s) PbI2 Precipitation reactions molecular equation ionic equation net ionic equation Na+ and NO3- arespectatorions CHE 131 - Chapter 4

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