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Solubility and Net Ionics

Solubility and Net Ionics. Solubility Rules. Most alkali metal salts AND NH₄⁺ salts are soluble All nitrates, chlorates, perchlorates, and acetates are soluble Cl ⁻, Br⁻, and I⁻ are soluble , EXCEPT Ag⁺, Hg₂⁺², Pb⁺² ( Pb halides are soluble in hot water)

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Solubility and Net Ionics

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  1. Solubility and Net Ionics

  2. Solubility Rules • Most alkali metal salts AND NH₄⁺ salts are soluble • All nitrates, chlorates, perchlorates, and acetates are soluble • Cl⁻, Br⁻, and I⁻ are soluble, EXCEPT Ag⁺, Hg₂⁺², Pb⁺² (Pb halides are soluble in hot water) • F⁻ are soluble, EXCEPT for IIA metals • All SO₄⁻² are soluble EXCEPT for Ca⁺², Sr²⁺, Ba²⁺, Ag⁺, Pb²⁺, and Hg₂⁺²

  3. Solubility Rules cont. 6. CO₃⁻², PO₄⁻³, C₂O₄⁻², CrO₄⁻², S⁻², OH⁻, and O⁻² are INSOLUBLE, except for group 1A metals.

  4. Exercise: Using the solubility rules, predict what will happen when the following pairs of solutions are mixed • KNO₃ (aq) and BaCl₂ (aq) nothing …. All the ions remain dissolved in solution. No chemrxn occurs 2. Na₂SO₄(aq) and Pb(NO₃)₂(aq) NaNO₃ is soluble, but PbSO₄ is insoluble and will precipitate from solution 3. KOH(aq) and Fe(NO₃)₃(aq) KNO₃ goes into solution, Fe(OH)₃ will form ppt.

  5. Net Ionics • COMPLETE balance equation gives overall rxnstoich, but NOT the forms of the rea and pro as they exist in solution • 2KI(aq) + Pb(NO₃)₂(aq)  2KNO₃(aq) + PbI₂(s) • Complete Ionic Equation represents as IONS all rea and pro that are strong electrolytes • K⁺ + I⁻ + Pb⁺² + NO₃⁻  K⁺ + NO₃⁻ + PbI₂(s) • Net Ionic Equations includes only those solution components undergoing change. • Spectator ions are those not involved in the rxn, thus not included in the NIE. • I⁻ + Pb⁺²  PbI₂(s)

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