CHEM 101 1nd Edition Lecture 17Outline of Last Lecture I. Limiting ReagentII. Concentration and MolarityOutline of Current Lecture I. pH: Potential HydrogenII. pH and [H+]III. Determining the Concentration of an Unknown Acid or Base Solution via TitrationCurrent LectureI. pH: Potential Hydrogena. Acidity is measured in terms of [H3O+]i. Typically ranges from 1 to 1 x 10-14 Mb. pH = - log [H3O+]i. Typically ranges from 0 to 14ii. pH < 7 is acidiciii. pH > 7 is basicII. pH and [H+]a. Because pH = - log [H+] then, log [H+] = - pHi. Take antilog and get: [H+] = 10-pHb. Neutralization:i. An acid and a base react to form water and a dissolved saltii. Equivalence pout is when there is an equal amount of acid and baseiii. Equivalence point for a strong acid – strong bade titration is at pH = 7.0III. Determining the Concentration of an Unknown Acid or Base Solution via Titrationa. Titrationi. A known concentration of base (or acid) is slowly added to a known volume of the acid (or base) of unknown concentration.ii. A Buret allows accurate determination of volume added of solution with known concentrationiii. Oxidation-reduction is another type of titrationb. How to Measure pH?i. pH metersii. pH indicationsiii. Litmus PaperThese 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.c. Acid-Base Titration Curvesi. pH change (Y-axis) as a function of the amount of acid or base added (X-axis)ii. Equivalence point is reached when there is an equal amount of acid and base1. When a pH meter is unavailable, an indicator can be used to determine when the solution has reached the equivalence pointa. Indicator changes color as the pH
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