2 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 Termsppt spectator ion
3 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.solubleinsolublesolute
4 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 reactionsDRDRSpectator ions - do not participate, remain moving freely in solution.
5 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.
7 NaCl(aq) + KBr(aq) NaBr(aq) + KCl(aq) Using the Solubility rules:*Assuming the reactants will dissolve…1. Predict the products of the reactionCheck RULES to see if each product will pptNaCl(aq) + KBr(aq)NaBr(aq) + KCl(aq)KBr (s) K+ (aq) + Br - (aq)NaCl (s) Na+ (aq) + Cl- (aq)
8 Indicate if any of the product form a precipitate (ppt). KOH (aq) + AgNO3 (aq)KNO3 (aq) + AgOH (aq)pptCalcium nitrate + sodium carbonateCa(NO3)2 + Na2CO3CaCO NaNO32ppt
9 Indicate if any of the product form a precipitate (ppt). Na2SO4 (aq) + KCl (aq)22 NaCl (aq) + K2SO4 (aq)Iron (III) chloride + lead (II) nitrateFeCl Pb(NO3)2232 Fe(NO3) PbCl2ppt
10 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 ionsThe net ionic equation shows the actual reaction that occurs – no spectators:Ag+(aq) + Cl−(aq) → AgCl(s)
11 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) KI(aq) → PbI2(s) KNO3(aq)Pb2+(aq) + 2 I−(aq) → PbI2(s)K+NO3−Spectator ions
12 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 Termsppt spectator ion