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Chapter 4

Chapter 4. Chemical Reactions. Solubility Rules. 1. All nitrates are soluble. 2. All compounds of Group IA metals and the ammonium ion, NH 4 + , are soluble. 3. All halides are soluble except: AgX, Hg 2 X 2 and PbX 2 , where X may be Cl, Br, or I.

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Chapter 4

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  1. Chapter 4 Chemical Reactions Dr. S. M. Condren

  2. Solubility Rules 1. All nitrates are soluble. 2. All compounds of Group IA metals and the ammonium ion, NH4+, are soluble. 3. All halides are soluble except: AgX, Hg2X2 and PbX2, where X may be Cl, Br, or I. 4. All sulfates are soluble except: PbSO4, BaSO4, and SrSO4. Dr. S. M. Condren

  3. Solubility Rules 5. All hydroxides and sulfides are insoluble except those of the Group IA metals and the ammonium ion. 6. All carbonates and phosphates are insoluble except those of the Group IA metals and the ammonium ion. Dr. S. M. Condren

  4. A solution of Ba(NO3)2 is added to a solution of Na2SO4 to make a precipitate. From a table of solubility rules, the product is barium sulfate, sodium nitrate Dr. S. M. Condren

  5. Electrolytes • Conduct electricity in solution due to the presence of ions • Strong electrolyte – completely ionized in solution • Weak electrolyte – partially ionized in solution • Non-electrolyte – nonionic solution Dr. S. M. Condren

  6. Water Conductivity Dr. S. M. Condren

  7. Strong Electrolyte Dr. S. M. Condren

  8. Weak Electrolyte Dr. S. M. Condren

  9. Chemical Equations Molecular Equation AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) Complete or Total Ionic Equation Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  AgCl(s) + Na+(aq) + NO3-(aq) Net Ionic Equation Ag+(aq) + Cl-(aq) AgCl(s) Dr. S. M. Condren

  10. Types of Reactions • synthesis reactions or combination reactions • decomposition reactions • precipitation reactions • neutralization reactions • acid • base • oxidation-reduction reaction Dr. S. M. Condren

  11. Precipitation Reactions The process of separating a substance from a solution as a solid. AgNO3 + NaCl ---> AgCl + NaNO3 precipitate Dr. S. M. Condren

  12. Neutralization Reactions • acid • base • salt Household acids and Bases Dr. S. M. Condren

  13. Neutralization Reactions • acid • Any of a large class of sour-tasting substances whose aqueous solutions are capable of turning blue litmus indicators red, of reacting with and dissolving certain metals to form salts, and of reacting with bases or alkalis to form salts. • Substance that donates H+ ions to solution Dr. S. M. Condren

  14. Neutralization Reactions • base • Any of a large class of compounds, including the hydroxides and oxides of metals, having a bitter taste, a slippery solution, the ability to turn litmus blue, and the ability to react with acids to form salts. • Substance that donates a OH-1 ion to solution Dr. S. M. Condren

  15. Neutralization Reactions • salt • The term salt is also applied to substances produced by the reaction of an acid with a base, known as a neutralization reaction. • Salts are characterized by ionic bonds, relatively high melting points, electrical conductivity when melted or when in solution, and a crystalline structure when in the solid state. Dr. S. M. Condren

  16. Neutralization Reactions acid + base ---> “salt” + water Dr. S. M. Condren

  17. Neutralization Reactions acid + base ---> “salt” + water HCl + NaOH ---> NaCl + H2O Dr. S. M. Condren

  18. Neutralization Reactions acid + base ---> “salt” + water H2SO4 + 2KOH ---> K2SO4 + 2H2O Dr. S. M. Condren

  19. Strong vs. Weak Acids and Bases • strong - completely ionized • weak - partially ionized Dr. S. M. Condren

  20. Oxidation-Reduction Reaction Oxidation - loss of electrons Reduction - gain of electrons Redox reaction oxidizing agent - substance that causes oxidation reducing agent - substance that cause reduction Dr. S. M. Condren

  21. Synthesis or Combination Reactions Formation of a compound from simpler compounds or elements. Dr. S. M. Condren

  22. Decomposition Reactions Separation into constituents by chemical reaction. Dr. S. M. Condren

  23. Electrolysis • decomposition caused by an electric current • anode • electrode where oxidation occurs • cathode • electrode where reduction occurs Dr. S. M. Condren

  24. Identify the oxidizing agent in the reaction: 2Al(s) + 6 H+ ==> 2 Al3+(aq) + 3 H2(g) Al, H+, Al3+, H2 Identify the oxidizing agent in the reaction: Dr. S. M. Condren

  25. Oxidation StatesRules for Assigning Oxidation States 1. zero for uncombined element 2. charge on monatomic ion 3. F is always -1; other halogens -1 except when combined with more electronegative halogen or oxygen Dr. S. M. Condren

  26. Oxidation StatesRules for Assigning Oxidation States 4. H is +1 except in metal hydrides, where H is -1 5. O is -2 except when combined with F (then +1 or +2) or in peroxides, -1. 6. sum of oxidation states equals charge on ion or molecule Dr. S. M. Condren

  27. Oxidation State What is the oxidation state of S in H2SO4? • H => +1 • O => -2 • neutral compound, thus sum equals zero • 4O => 4*-2 = -8 • 2H => 2*+1 = +2 • 0 = +2 + (x) + (-8) x = +6 Dr. S. M. Condren

  28. Oxidation State What is the oxidation state of Cl in HClO4? • H => +1 • O => -2 • neutral compound, thus sum equals zero • 4O => 4*-2 = -8 • H => 1*+1 = +1 • 0 = +1 + (y) + (-8) y = +7 Dr. S. M. Condren

  29. Activity Series of Metals • Highest metal in series is the most reactive • A reactive metal will react with ions of less reactive metal to produce ions of reactive metal and atoms of the less reactive metal Dr. S. M. Condren

  30. Metal Reaction with Acid Dr. S. M. Condren

  31. Single Displacement Dr. S. M. Condren

  32. 2Cu(s) + O2 (g) ---> 2CuO(s) The oxidation number of copper in the product is Cu(0), Cu(I), Cu(II) In the reaction, copper metal is reduced, oxidized, unchanged in oxidation state Dr. S. M. Condren

  33. Solution Solutions, in chemistry, homogeneous mixtures of two or more substances. Dr. S. M. Condren

  34. Solute The substance that is present in smallest quantity is said to be dissolved and is called the solute. The solute can be either a gas, a liquid, or a solid. Dr. S. M. Condren

  35. Solvent The substance present in largest quantity usually is called the solvent. The solvent can be either a liquid or a solid. Dr. S. M. Condren

  36. Preparation of a Solution Dr. S. M. Condren

  37. Molarity The number of moles of solute per liter of solution. molarity => M moles of solute M = -------------------- liter of solution units => molar = moles/liter = M Dr. S. M. Condren

  38. EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH? 2 NaOH(aq) + H2SO4(aq) -----> Na2SO4(aq) + 2 H2O Dr. S. M. Condren

  39. EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH? 2 NaOH(aq) + H2SO4(aq) -----> Na2SO4(aq) + 2 H2O (25.0 mL NaOH) #mL H2SO4 = ---------------------- Dr. S. M. Condren

  40. EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH? 2 NaOH(aq) + H2SO4(aq) -----> Na2SO4(aq) + 2 H2O (25.0 mL NaOH) (0.400 mol NaOH) #mL H2SO4 = --------------------------------------------- (1 L NaOH) Dr. S. M. Condren

  41. EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH? 2 NaOH(aq) + H2SO4(aq) -----> Na2SO4(aq) + 2 H2O (25.0 mL NaOH) (0.400 mol NaOH)(1 L) #mL H2SO4 = ------------------------------------------------------- (1 L NaOH) (1000 mL) Dr. S. M. Condren

  42. EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH? 2 NaOH(aq) + H2SO4(aq) -----> Na2SO4(aq) + 2 H2O (25.0) (0.400 mol NaOH)(1) (1 mol H2SO4) #mL H2SO4 = ------------------------------------------------------ (1) (1000) (2 mol NaOH) Dr. S. M. Condren

  43. EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH? 2 NaOH(aq) + H2SO4(aq) -----> Na2SO4(aq) + 2 H2O (25.0)(0.400)(1 mol H2SO4)(1000 mL H2SO4) #mL H2SO4 = -------------------------------------------------------- (1) (1000) (2) (0.200 mol H2SO4) Dr. S. M. Condren

  44. EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH? 2 NaOH(aq) + H2SO4(aq) -----> Na2SO4(aq) + 2 H2O (25.0)(0.400)(1)(1000 mL H2SO4) #mL H2SO4 = ------------------------------------------ (1) (1000) (2) (0.200) Dr. S. M. Condren

  45. EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH? 2 NaOH(aq) + H2SO4(aq) -----> Na2SO4(aq) + 2 H2O (25.0)(0.400)(1)(1000 mL H2SO4) #mL H2SO4 = ------------------------------------------ (1) (1000) (2) (0.200) = 25.0 mL H2SO4 Dr. S. M. Condren

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