CHEM 122 11th Edition Lecture 26 Outline of Last LectureI. Strong Basesa. Properties of binary oxidesII. Lewis Acids and BasesIII. Autoionization of WaterIV. pH Scale for Acids and BasesOutline of Current Lecture I. Acid/Base ionization Constant a. Strength of acids and bases b. Calculations of weak acid and base solutionsCurrent LectureAcid/Base Ionization Constants - Acid (Ka)/base (Kb) ionization constant: equilibrium constant for a weak acid/base. - General equation for weak acid dissociation:−¿(aq)+¿(aq)+A¿HA(aq)❑⇔H¿- General equation for base ionization constant: −¿(aq)+¿(aq)+O H¿B(aq)+H2O(l)❑⇔B H¿- The magnitude of acid/base ionization constants is a measure of the strength of the acid/base. If Kb is bigger than Ka, then the base is stronger base than the acid.- In addition to the ionization constants, the strength could be measured by the p-function. - Stronger acid, larger Ka value, smaller pKa value. (same for bases)- For any conjugate acid-base pair: Ka x Kb = Kw =1.0x10^-14These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best Used as a supplement to your own notes, not as a substitute.- As Ka increases, Kb for the conjugate base must decrease.- Calculations of weak acid and base solutions:o calculate Ka or Kb from initial concentration of acid or base and the known of pH [H+] of the solutiono calculate equilibrium concentrations given Ka or Kb and initial concentrations. Write out the equilibrium law and create an ICE table to find the equilibrium concentrations.o Substitute the equilibrium concentrations expression into the Ka expression to find
View Full Document
Unlocking...