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Chapter 4 Reactions in Aqueous Solution

Chapter 4 Reactions in Aqueous Solution. Naming Chemical Compounds. Binary Acids Hydrogen + nonmetal (no oxygen) Naming: Hydro +root of lement+ ic acid ending. HCl hydro chlor ic acid HBr hydro brom ic acid HF hydro fluor ic acid. *Exception: HCN – hydrocyanic acid.

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Chapter 4 Reactions in Aqueous Solution

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  1. Chapter 4Reactions in Aqueous Solution

  2. Naming Chemical Compounds Binary Acids Hydrogen + nonmetal (no oxygen) Naming: Hydro+root of lement+ic acid ending HCl hydrochloric acid HBr hydrobromic acid HF hydrofluoric acid *Exception: HCN – hydrocyanic acid

  3. Naming Chemical Compounds No hydro- prefix Root of polyatomic anion + ous acid ending Or ic acid ending Polyatomic anion “ous” “ite” “ic” “ate”

  4. Examples • Name the following acids • H2S • H2CO3 • HBrO3 • H3PO3

  5. AgNO3(aq) + NaCl(aq) NaNO3(aq) + AgCl(s) Some Ways That Chemical Reactions Occur Precipitation Reactions: Processes in which soluble reactants yield an insoluble solid product that falls out of solution.

  6. HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq) Some Ways That Chemical Reactions Occur Acid-Base Neutralization Reactions: Processes in which an acid reacts with a base to yield water plus a salt. Acid + Base  Water + Salt

  7. Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g) Some Ways That Chemical Reactions Occur Oxidation-Reduction (Redox) Reactions: Processes in which one or more electrons are transferred between reaction partners (atoms, molecules, or ions). Element + Compound  Compound + Element Neutral state: (s), (l), (g)

  8. Electrolytes

  9. C12H22O11(s) C12H22O11(aq) CH3CO2H(aq) H1+(aq) + CH3CO21-(aq) H2O Electrolytes in Aqueous Solution Strong Electrolytes: Compounds that dissociate to a large extent into ions when dissolved in water. KCl(aq) K1+(aq) + Cl1-(aq) Weak Electrolytes: Compounds that dissociate to a small extent into ions when dissolved in water. Nonelectrolytes: Substances which do not produce ions in aqueous solutions.

  10. Electrolytes in Aqueous Solution Memorize these acids Strong Acids: hydrochloric acid, hydrobromic acid, hydroiodic acid, perchloric acid, nitric acid, sulfuric acid.

  11. Electrolytes in Aqueous Solution Ionic Compounds

  12. Electrolytes in Aqueous Solution Weak acids

  13. Electrolytes in Aqueous Solution Molecular Compounds (other than any strong or weak electrolytes)

  14. AgNO3(aq) + NaCl(aq) NaNO3(aq) + AgCl(s) Aqueous Reactions and Net Ionic Equations Molecular Equation: All substances in the chemical equation are written using their complete formulas as if they were molecules. Precipitate insoluble strong electrolytes indicated as (aq) soluble

  15. Aqueous Reactions and Net Ionic Equations Ionic Equation: All of the strong electrolytes are written as ions. AgNO3(aq) NaCl(aq) Ag2+(aq) + NO31- (aq) + Na1+(aq) + Cl1-(aq) Na1+(aq) + NO31- (aq) + AgCl(s) NaNO3(aq)

  16. Aqueous Reactions and Net Ionic Equations Spectator Ions: Ions that undergo no change during the reaction and appear on both sides of the reaction arrow. Ag2+(aq) + NO31- (aq) + Na1+(aq) + Cl1-(aq) Na1+(aq) + NO31- (aq) + AgCl(s)

  17. Ag+(aq) + Cl1-(aq) AgCl2(s) Aqueous Reactions and Net Ionic Equations Net Ionic Equation: Only the ions undergoing change are shown.

  18. Precipitation Reactions and Solubility Guidelines

  19. AB + CD CB + AD Precipitation Reactions and Solubility Guidelines Write the chemical formulas of the products (use proper ionic rules). double replacement reaction *Remember that metal cation does not bond to another metal cation

  20. Precipitation Reactions and Solubility Guidelines Write the molecular, ionic, and net ionic equations for the reaction that occurs when aqueous solutions of Iron(III) nitrate and Sodium Hydroxide are mixed.

  21. Example • Write the molecular, ionic, and net ionic equations for the reaction that occurs when • aqueous solutions of PbCl2 and Na2SO4 are mixed • Aqueous solution of Mg(NO3)2 and NH4OH

  22. HCl(aq) + H2O(aq) HCl(aq) HA(aq) H3O1+(aq) + Cl1-(aq) H1+(aq) + A1-(aq) H1+(aq) + Cl1-(aq) Acids, Bases, and Neutralization Reactions Acid (Arrhenius): A substance that dissociates in water to produce hydrogen ions, H1+: In water, acids produce hydronium ions, H3O1+:

  23. NH3(aq) + H2O(aq) NaOH(aq) MOH(aq) M1+(aq) + OH1-(aq) Na1+(aq) + OH1-(aq) NH41+(aq) + OH1-(aq) Acids, Bases, and Neutralization Reactions Base (Arrhenius): A substance that dissociates in water to produce hydroxide ions, OH1-: Ammonia, commonly called “ammonium hydroxide” is a base:

  24. Acids, Bases, and Neutralization Reactions Strong acids andstrong bases are strong electrolytes. Weak acids and weak bases are weak electrolytes.

  25. HA + MOH HA + MOH MA + H2O MA + HOH Acids, Bases, and Neutralization Reactions These acid-base neutralization reactions are double-replacement reactions just like the precipitation reactions: or Acid Base Salt Water

  26. Acids, Bases, and Neutralization Reactions • Write the molecular, ionic, and net ionic equations for the reaction of aqueous H2SO4 and aqueous KOH

  27. Acids, Bases, and Neutralization Reactions Write the molecular, ionic, and net ionic equations for the reaction of aqueous NaOH and aqueous HF.

  28. Examples • Predict the product and write a molecular equation, ionic equation and net ionic equation for the following reactions • K2CO3(aq) + CuCl2(aq)  • HNO3(aq) + LiOH(aq)  • H2SO3(aq) + NaOH 

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