CEM142 1nd Edition Lecture 11 Outline of Last Lecture I. Acid titrationsII. Base titrationsOutline of Current Lecture II. Acid/base titrations continuedIII. Solubility Current Lecture-review-titration: neutralization-Henderson Hasselbach equation-pH = pKa + log ([A-]/[HA])-A- = conjugate base-HA = acid-at the halfway point…-[A-] = [HA]-therefore pH = pKa because log(1)=0-at the equivalent point…-number of moles of A- = number of moles of HA-polyprotic acids: acids that can donate more than 1 H+ to either water or to a base-examples: H3PO4, H2SO4, H2SO3, H2CO3-removing the first hydrogen is always easier than removing the second hydrogen-example: These 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.1. H2CO3 + H2O HCO3- + H3O+2. HCO3- + H2O CO32- + H3O+-the first step is easier and occurs faster than the second step-heterogeneous equilibria: 2 or more different phases involved-example: dissolving a salt (solid) in a solvent (aqueous)-saturation: occurs when the maximum amount of salt is dissolved into solution, you cankeep adding more but it won’t
View Full Document
Unlocking...