Solubility Rules. The terms soluble and insoluble are relative terms. soluble insoluble solute Solubility: the maximum amount of solute needed to make.

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Presentation transcript:

Solubility Rules

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

Basis Solubility Rules 1.All ionic compounds containing Group 1 elements, H + and ammonium ion are soluble. 2.All ionic compounds with Group VII elements (other than F) and metals are soluble, except those of Ag +, Hg +1, and Pb All acetates and nitrates are soluble. 4.All sulfates are soluble except those of Ba +, Sr +2, Pb +2, Ca +2, Ag +, Hg Carbonates, hydroxides, oxides, sulfides, phosphates, chromates and dichromates are soluble; ONLY when bonded with those in rule 1.

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) NaCl (s) Na + (aq) + Cl - (aq) KBr (s) K + (aq) + Br - (aq) NaBr (aq) + KCl (aq)

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

Indicate if any of the product form a precipitate (ppt). KOH (aq) + AgNO 3 (aq) Calcium nitrate + sodium carbonate KNO 3 (aq) + AgOH (aq) Ca(NO 3 ) 2 + Na 2 CO 3 CaCO 3 + NaNO 3 ppt 2

Indicate if any of the product form a precipitate (ppt). Na 2 SO 4 (aq) + KCl (aq) Iron (III) chloride + lead (II) nitrate 2 NaCl (aq) + K 2 SO 4 (aq) 2 FeCl 3 + Pb(NO 3 ) Fe(NO 3 ) PbCl 2 2 ppt

AgNO 3(aq) + NaCl (aq) → AgCl (s) + NaNO 3(aq) The complete ionic equation shows all ions in their dissociated form. Ag + (aq) + NO 3 − (aq) + Na + (aq) + Cl − (aq) → AgCl (s) + Na + (aq) + NO 3 − (aq) The net ionic equation shows the actual reaction that occurs – no spectators: Ag + (aq) + Cl − (aq) → AgCl (s) Spectator ions

Write the molecular equation and the net ionic equation for the reaction between aqueous lead (II) nitrate and aqueous potassium iodide. Pb(NO 3 ) 2(aq) + 2 KI (aq) → PbI 2(s) + 2 KNO 3(aq) Pb 2+ (aq) + 2 I − (aq) → PbI 2(s) Spectator ions K+K+ NO 3 −