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Solubility Rules

Solubility Rules. Solubility: the maximum amount of solute needed to make a saturated solution , under given conditions. The terms soluble and insoluble are relative terms. solute. insoluble. soluble. soluble. Basis Solubility Rules

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Solubility Rules

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  1. Solubility Rules

  2. Solubility: the maximum amount of solute needed to make a saturated solution, under given conditions. The terms soluble and insoluble are relative terms. solute insoluble soluble soluble

  3. Basis Solubility Rules All ionic compounds containing Group 1 elements, H+ and ammonium ion are soluble. All ionic compounds with Group VII elements (other than F) and metals are soluble, except those of Ag+, Hg+1, and Pb+2. All acetates and nitrates are soluble. All sulfates are soluble except those of Ba+, Sr+2, Pb+2, Ca+2, Ag+, Hg+1. 5. Carbonates, hydroxides, oxides, sulfides, phosphates, chromates and dichromatesare soluble; ONLY when bonded with those in rule 1.

  4. NaCl (s) Na+(aq) + Cl- (aq) KBr (s) K+(aq) + Br - (aq) Using the Solubility rules: 1. Predict whether a solute will dissolve in water. 2. Predict when a ppt will form during a reaction. NaCl(aq) + KBr(aq) NaBr(aq) + KCl(aq)

  5. Precipitation reactions: The formation of an ioniccompound that is not soluble in the current solvent. Spectator ions - do not participate, remain moving freely in solution.

  6. KOH (aq) + AgNO3(aq) Ca(NO3)2 + Na2CO3 Calcium nitrate + sodium carbonate Indicate if any of the product form a precipitate (ppt). KNO3(aq) + AgOH (aq) ppt CaCO3 + NaNO3 2 ppt

  7. Na2SO4(aq) + KCl (aq) FeCl3 + Pb(NO3)2 Iron (III) chloride + lead (II) nitrate Indicate if any of the product form a precipitate (ppt). 2 2 NaCl (aq) + K2SO4 (aq) 2 3 2 Fe(NO3)3 + 3 PbCl2 ppt

  8. AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) The complete ionic equation shows all ions in their dissociated form. Ag+(aq) + NO3−(aq) + Na+(aq) + Cl−(aq) → AgCl(s)+ Na+(aq) + NO3−(aq) Spectator ions The net ionic equation shows the actual reaction that occurs – no spectators: Ag+(aq) + Cl−(aq) → AgCl(s)

  9. Write the molecular equation and the net ionic equation for the reaction between aqueous lead (II) nitrate and aqueous potassium iodide. Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq) Pb2+(aq) + 2 I−(aq) → PbI2(s) K+ NO3− Spectator ions

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