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Chapter Four – Part 2

Chapter Four – Part 2. Chemical Reactions in Aqueous Solutions. Net Ionic Equations. In many reactions (acid-base, precipitation, some others) the reacting species are not molecules, but ions . The equation: AgNO 3 (aq) + KCl(aq)  AgCl(s) + KNO 3 (aq)

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Chapter Four – Part 2

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  1. ChapterFour – Part 2 Chemical Reactions in Aqueous Solutions

  2. Net Ionic Equations • In many reactions (acid-base, precipitation, some others) the reacting species are not molecules, but ions. • The equation: AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq) is misleading because the species that actually react aren’t AgNO3 and KCl. They are ____ and ____

  3. Net Ionic Equations • In a net ionic equation, only the species that actually react and are formed are shown. • Spectator ions that “sit on the sidelines” are left out of the equation. • AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq) Spectator ions • Ag+ + NO3– + K+ + Cl– AgCl(s) + K+ + NO3– • Ag+ + Cl– AgCl(s) (Net ionic) These ions react

  4. To Write a Net Ionic Equation • Write the balanced equation. [Molecular Equation] • Identify the strong and soluble electrolytes and dissociate them (strong soluble electrolytes = dissociate completely) [Ionic Equation] • Cancel spectator ions (identical on both sides of the equation). [Net Ionic Equation] 2 CH3COOH(aq) + Ba(OH)2 (aq)  Ba(CH3COO)2+ 2 H2O(aq) 2 CH3COOH + Ba2+ + 2 OH– Ba2+ + 2 CH3COO– + 2 H2O 2 CH3COOH + 2 OH– 2 CH3COO– + 2 H2O (Net ionic) or CH3COOH + OH– CH3COO– + H2O (Net ionic)

  5. Review: Dissociating Ionic Compounds Q - Write the ions that form from Al2(SO4)3(aq)?

  6. Practice with writing ions Q - Write ions for Na2CO3(aq) Q - Write ions for Ca3(PO4)2(aq) Q - Write ions for Mg3(BO3)2(aq)

  7. Equations must be balanced • There are two conditions for molecular, ionic, and net ionic equations Materials balance Both sides of an equation should have the same number of each type of atom Electrical balance Both sides of a reaction should have the same net charge Q- When NaOH(aq) and MgCl2(aq) are mixed, _______(s) and NaCl(aq) are produced. Write balanced molecular, ionic & net ionic equations Mg(OH)2

  8. NaOH(aq) + MgCl2(aq)  Mg(OH)2(s) + NaCl(aq) 2 2 First write the molecular equation Ionic equation: 2Na+(aq) + 2OH-(aq) + Mg2+(aq) + 2Cl-(aq)  Mg(OH)2(s) + 2Na+(aq) + 2Cl-(aq) Net ionic equation: 2OH-(aq) + Mg2+(aq)  Mg(OH)2(s)

  9. Write balanced ionic and net ionic equations: CuSO4(aq) + BaCl2(aq) 

  10. Write balanced ionic and net ionic equations: Fe(NO3)3(aq) + LiOH(aq)  Na3PO4(aq) + CaCl2(aq)  Na2S(aq) + AgC2H3O2(aq) 

  11. Fe3+(aq) + 3NO3–(aq) + 3Li+(aq) + 3OH–(aq)  3Li+(aq) + 3NO3–(aq) + Fe(OH)3(s) Net: Fe3+(aq) + 3OH–(aq)  Fe(OH)3(s) 6Na+(aq) + 2PO43–(aq) + 3Ca2+(aq) + 6Cl–(aq)  Ca3(PO4)2(s)+ 6Na+(aq) + 6Cl–(aq) Net: 2PO43–(aq) + 3Ca2+(aq)  Ca3(PO4)2(s) 2Na+(aq) + S2–(aq) + 2Ag+(aq) + 2C2H3O2–(aq)  2Na+(aq) + 2C2H3O2–(aq) + Ag2S(s) Net: S2–(aq) + 2Ag+(aq)  Ag2S(s)

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