CEM142 1nd Edition Lecture 9 Outline of Last Lecture I. Bronsted-Lawry Acids and BasesOutline of Current Lecture II. Hydrolysis of saltsIII. Polyprotic acidsIV. Polyprotic basesCurrent Lecture-review:-acid: H+ donor-HA + H2O A- + H3O+-Ka = [A-][H3O+]/[HA]-pKa = -logKa-base: H+ acceptor-B + H2O BH+ + OH--Kb = [BH+][OH-]/[B]-pKb = -logKb-example problem: what does NaCl do in water?-Na+(aq) + Cl-(aq)-Cl--Cl-(base) + H2O(acid) HCl(conjugate acid) + OH-(conjugate base)-HCl is a very strong acid-OH is a stronger base than ClThese 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.-equilibrium is pushed to the left so the equation looks like…Cl-(base) + H2O(acid) HCl(conjugate acid) + OH-(conjugate base)-so Cl does not react with water because HCl is so strong that it pushes equilibrium 100% to the left-Na+-it doesn’t have a H to donate so it can’t be an acid-Na+ and H+ have the same charge so they repel each other, and therefore Na can’t act as a base
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