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Solubility Rules

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. Solubility:

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Solubility Rules

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  1. Solubility Rules

  2. Explainexamples of solubility and precipitation at both the particle and symbolic levels. • Usea table of solubility rules to predict the formation of a precipitate. • Additional KEY Terms • ppt spectator ion

  3. Solubility: The amountof solute needed to make a saturatedsolution, under given conditions. The terms soluble and insoluble are relative terms. solute insoluble soluble soluble

  4. Precipitation (ppt) reaction: Formationof an ioniccompound 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.

  5. 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 dichromatesare soluble; ONLY when bonded with those in rule 1.

  6. Basic Solubility Rules (View 2)

  7. NaCl (s) Na+(aq) + Cl- (aq) KBr (s) K+(aq) + Br - (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)

  8. 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

  9. 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

  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 ions The net ionic equation shows the actual reaction that occurs – no spectators: Ag+(aq) + Cl−(aq) → AgCl(s)

  11. 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

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

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