Unit 6
Acids/Bases and Aqueous Equilibriums
Unit Calendar
Chapter 16: Acid-Base Equilibria
16.1+2 Acid and bases and bronsted-lowry acids and bases
describe the Arrhenius definition of acids/bases
describe acids and bases and their reactions in terms of proton-transfers
identify acids/bases and their conjugate bases/acids
describe what it means to be a strong/weak acid/base as well as the corresponding strengths of their conjugate base/acid
16.3+4 autoionization of water +pH Scale
16.5 strong acids and bases
Explain what makes a ‘strong’ acid/base ‘strong.
Identify the common strong acids and bases
determine the pH of solutions based on the strong acid/base concentration
16.6 weak acids
16.7 weak bases
16.8 relationship between Ka and Kb
convert between Ka and Kb (optional: video)
16.9 acid-base properties of salt solutions
predict a salt's effect on pH based on the cation and anions present (optional: video)
16.10 acid-base behavior and chemical structure
predict/compare the strength of various acids/bases based on their chemical structures
16.11 Lewis acids and bases
Classify compounds as lewis acids/bases based on how they react. (optional: video)
predict whether ‘X’ or ‘Y’ would be a stronger lewis acid/base based on its chemistry
Chapter 16 Resources
Chapter 17: Other Aspects of Aqueous Equilibrium
17.1 the common ion effect
Explain the influence of common ions on solution equilibriums.(think Le Chatelier's principle)
Determine the pH of a solution containing an ionic compound with the conjugate of a weak acid or base with that acid/base
17.2 buffered solutions
Explain what a buffered solution is and how they resist changes in pH (optional: Video)
Explain the concept of buffer capacity (optional:video)
Use the Henderson-Hasselbalch equation to determine the properties of a buffered solution (pH, concentration of acid/base, Ka, response to addition of acids or bases) (optional:video 1, video2)
17.3 acid-base titration
Experimentally determine a solution's concentration by titration
explain how the equivalence point and titration curves vary when titrating a weak acid/base and polyprotic acids
Calculate pH for a mixture of an acid and a base
17.4 solubility equilibria
Use the Ksp expression to determine ion concentration and molar solubility and vice versa
17.5 factors that affect solubility
calculate molar solubilities of a salt in a solution containing a common ion
Analyze the effect of pH on the solubility of various compounds
Analyze how the formation of complex ions affects the solubility of various compounds
17.6 precipitation and separations of ions
17.7 qualitative analysis for metallic elements
Objectives:
Apply the differences in solubilities to create a systematic means of qualitatively analyzing mixtures
Chapter 17 Resources