Chem Ii Study Guide
Multiple Choice: (42 points)
Chapter 15: Principles of Chemical Equilibrium
dynamic equilibrium equilibrium constant reversibility LeChâtelier’s Principle ICE table Q and Keq major species minor species Keq,f vs Keq,r rate constant vs. equilibrium expressions significance of magnitude of Keq equilibrium shift with concentration changes equilibrium shift with temperature changes equilibrium shift with volume changes Chapter 16: Acid-Base Euilibrium Brønsted-Lowry acid Brønsted-Lowry base amphoteric water equilibrium constant pH pOH pH scale weak acid Ka and pKa weak base Kb and pKb oxyacids carboxylic acids polyprotic acids amines conjugate acid conjugate base pH of acidic salt solutions pH of basic salt solutions relate Ka and Kb acid strength (binary acids) acid strength (oxyacids) Lewis acid Lewis base Chapter 17: Additional Aspects of Aqueous Equilibria
common ion effect effect of buffer composition of buffer preparation of buffers Henderson-Hasselbach equation buffer capacity buffer range SA/SB titration curve WA/SB titration curve equivalence point pH at equivalence pt buffer region pH at midpoint solubility product constant insoluble Ksp slightly soluble Ksp soluble Ksp
Short problems: (about 45 points) 1. Calculate [H3O+] and [OH-] for a KOH solution with pH = 9.36.
------------------------------------------------- ------------------------------------------------- [H3O+] = [OH-] =
-------------------------------------------------
2. A container initially has 0.500 atm NO2. At equilibrium, the NO2 pressure is 0.186 atm. Calculate the value of Kp.
------------------------------------------------- ------------------------------------------------- Kp =
-------------------------------------------------
3. Determine the Ka or Kb for each of the following
Chapter 15: Principles of Chemical Equilibrium
dynamic equilibrium equilibrium constant reversibility LeChâtelier’s Principle ICE table Q and Keq major species minor species Keq,f vs Keq,r rate constant vs. equilibrium expressions significance of magnitude of Keq equilibrium shift with concentration changes equilibrium shift with temperature changes equilibrium shift with volume changes Chapter 16: Acid-Base Euilibrium Brønsted-Lowry acid Brønsted-Lowry base amphoteric water equilibrium constant pH pOH pH scale weak acid Ka and pKa weak base Kb and pKb oxyacids carboxylic acids polyprotic acids amines conjugate acid conjugate base pH of acidic salt solutions pH of basic salt solutions relate Ka and Kb acid strength (binary acids) acid strength (oxyacids) Lewis acid Lewis base Chapter 17: Additional Aspects of Aqueous Equilibria
common ion effect effect of buffer composition of buffer preparation of buffers Henderson-Hasselbach equation buffer capacity buffer range SA/SB titration curve WA/SB titration curve equivalence point pH at equivalence pt buffer region pH at midpoint solubility product constant insoluble Ksp slightly soluble Ksp soluble Ksp
Short problems: (about 45 points) 1. Calculate [H3O+] and [OH-] for a KOH solution with pH = 9.36.
------------------------------------------------- ------------------------------------------------- [H3O+] = [OH-] =
-------------------------------------------------
2. A container initially has 0.500 atm NO2. At equilibrium, the NO2 pressure is 0.186 atm. Calculate the value of Kp.
------------------------------------------------- ------------------------------------------------- Kp =
-------------------------------------------------
3. Determine the Ka or Kb for each of the following