Solubility Rules

Explain examples of solubility and precipitation at both the particle and symbolic levels.   Use a table of solubility rules to predict the formation of a precipitate. Additional KEY Terms ppt spectator ion

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

Usually SR or chemical reactions Precipitation (ppt) reaction: Formation of an ionic compound that is not soluble in the current solvent. Usually SR or chemical reactions DR DR Spectator ions - do not participate, remain moving freely in solution.

Basic Solubility Rules (View 1) There are many different ways to present RULES for what will dissolve and what will NOT (ppt) Basic Solubility Rules (View 1) 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 dichromates are soluble; ONLY when bonded with those in rule 1.

Basic Solubility Rules (View 2)

NaCl(aq) + KBr(aq) NaBr(aq) + KCl(aq) Using the Solubility rules: *Assuming the reactants will dissolve… 1. Predict the products of the reaction Check RULES to see if each product will ppt NaCl(aq) + KBr(aq) NaBr(aq) + KCl(aq) KBr (s) K+ (aq) + Br - (aq) NaCl (s) Na+ (aq) + Cl- (aq)

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

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

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)

Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq) 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

CAN YOU / HAVE YOU? Explain examples of solubility and precipitation at both the particle and symbolic levels.   Use a table of solubility rules to predict the formation of a precipitate. Additional KEY Terms ppt spectator ion