Chapter 4. Three Major Classes of Chemical Reactions

  • 4.7The Reversibility of Reactions and the Equilibrium State

Concepts and Skills to Review Before You Study This Chapter

  1. names and formulas of compounds (Section 2.8)
  1. nature of ionic and covalent bonding (Section 2.7)
  1. amount-mass-number conversions (Section 3.1)
  1. balancing chemical equations (Section 3.3)
  1. calculating quantities of reactants and products (Section 3.4)
  • 4.1Solution Concentration and the Role of Water as a Solvent
  • Polar Nature of Water
  • Ionic Compounds in Water
  • Strong/weak electrolytes
  • Moles of compound and moles of ions
  • Covalent Compounds in Water
  • Non electrolytes
  • Expressing Concentration in Terms of Molarity
  • M=mol/L
  • Amount-Mass-Number Conversions Involving Solutions
  • M, mol, L conversion
  • Preparing and Diluting Molar Solutions
  • M1V1=M2V2
  • 4.2Writing Equations for Aqueous Ionic Reactions
  • Molecular/total ionic/net ionic equations
  • Spectors
  • 4.3Precipitation Reactions
  • The Key Event: Formation of a Solid
  • Non(s)  (s)
  • Predicting Whether a Precipitate Will Form
  • Solubility ruels
  • Stoichiometry of Precipitation Reactions
  • 4.4Acid-Base Reactions
  • Strong/weak acids/bases
  • Strong/weak electrolytes
  • When writing ionic equations….
  • The Key Event: Formation of Water
  • Acids: H+ donor in water
  • Bases: OH- donor in water
  • Proton Transfer in Acid-Base Reactions
  • Acids: H+ donor in water
  • Bases: H+ acceptor in water
  • Stoichiometry of Acid-Base Reactions: Acid-Base Titrations
  • 4.5Oxidation-Reduction (Redox) Reactions
  • The Key Event: Movement of Electrons
  • Transfer of electrons to make ions
  • Shifting of electrons to make covalent compounds
  • Redox Terminology
  • Oxidation: losing electrons
  • Reduction: gaining electrons
  • Oxidizing agent:
  • Reducing agent:
  • Oxidation Numbers
  • Assign oxidation numbers
  • Stoichiometry of Redox Reactions: Redox Titrations
  • 4.6Elements in Redox Reactions
  • Combination Reactions
  • Decomposition Reactions
  • Displacement Reactions and Activity Series
  • Combustion Reactions
  1. Calculate the number of moles of solute in 1.875 L of 1.356 M NaOH solution.
  1. Calculate the mass of solute needed to prepare 1.575 L of 0.00250 M NaClO3 (= 106.45 g/mol).
  1. Calculate the molarity of a solution prepared by dissolving 1.495 moles of LiOH in enough water to give a final volume of 750. mL.
  1. What volume, in L, of 10.0 MHCl is needed to make 2.00 L of 2.00 MHCl solution by dilution with water?
  1. How many moles of ions are released when 1.6 mol of ammonium phosphate, (NH4)3PO4, is dissolved in water?
  1. How many sodium ions are present in 325 mL of 0.850 M Na2SO4? Sulfate ions? Total ions?

  1. Which of the following is a strong acid?

A) H3PO4 B) HNO3 C) HF D) CH3COOH E) H2O
  1. Which of the following is most soluble in water?

A) / benzene, C6H6 / D) / hexane, C6H14
B) / potassium nitrate, KNO3 / E) / ethane, C2H4
C) / carbon tetrachloride, CCl4
  1. Which of the following solutions will be the best conductor of electrical current from the choice above?
  1. Which one of the following ionic compounds is insoluble in water?

A) Na3PO4 B) AgNO3 C) NaCl D) CaCO3 E) MgCl2
  1. Which of the following solutions will be the worst conductor of electrical current from the choice above?
  1. Complete the reaction. Na2CO3(aq) + BaCl2(aq) 
  1. Pb(NO3)2(aq) + 2NaCl(aq)  PbCl2(s) + 2NaNO3(aq)
  2. Write the total ionic equation.
  1. Write the net ionic equation.
  1. Ba(OH)2(aq) + HNO3(aq) 
  1. LiOH(aq) + HBr(aq)  H2O(l) + LiBr(aq)
  1. How much 1.20 MNaOH will be needed to neutralize 225 mL of 3.0 M H2SO4?

H2SO4(aq) + 2NaOH(aq)  2H2O(l) + Na2SO4(aq)

  1. Vinegar is a solution of acetic acid, CH3COOH, dissolved in water. A 5.54-g sample of vinegar was neutralized by 30.10 mL of 0.100 MNaOH. What is the percent by weight of acetic acid in the vinegar?
  1. Assign oxidation number for each element in …

Na2S2O5Na5P3O10H2PO2–

H2SKClO4

  1. Hg2+(aq) + Cu(s)  Cu2+(aq) + Hg(l)

Reduced? Oxidized? Reducing agent? Oxidizing agent? Number of electrons lost? Gained? Transferred?

  1. 2S2O32–(aq) + I2(aq)  S4O62–(aq) + 2I–(aq)

Reduced? Oxidized? Reducing agent? Oxidizing agent? Number of electrons lost? Gained? Transferred?

  1. Name the reaction as many ways as possible.
  2. H2(g) + Cl2(g)  2HCl(g)
  3. H2CO3(aq)  H2O(l) + CO2(g)
  4. BaCl2(aq) + Na2SO4(aq)  BaSO4(s) + 2NaCl(aq)
  5. NH3(aq) + HNO3(aq)  NH4NO3(aq)