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CHEM 1212: Acids and Bases

by: Brittany Ariana Borzillo

CHEM 1212: Acids and Bases CHEM 1212L

Marketplace > University of Georgia > Chemistry > CHEM 1212L > CHEM 1212 Acids and Bases
Brittany Ariana Borzillo
GPA 3.7

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This 2 page Class Notes was uploaded by Brittany Ariana Borzillo on Thursday October 13, 2016. The Class Notes belongs to CHEM 1212L at University of Georgia taught by Stanton in Fall. Since its upload, it has received 5 views. For similar materials see /class/202560/chem-1212l-university-of-georgia in Chemistry at University of Georgia.


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Date Created: 10/13/16
Acids and Bases Molecular Structure and Control of Acid–Base Strength  Factors that control acid-strength o Molecules with weaker H-A bonds tend to be stronger acids. o Molecules in which the group of atoms (-A) attached to the acidic hydrogen has a high electron-accepting ability tend to be stronger acids. o additional electronegative oxygen atom increases the electron- accepting ability of the group, drawing electron density away from the Cl atom  electron-withdrawing effect, also known as the inductive effect, draws electron density away from the oxygen atom bonded to the acidic hydrogen and makes it easier to remove H (as H+) from the OH group  As the number of electronegative, electron-withdrawing atoms increases in a series of oxoacids, it becomes easier to lose H+ from the OH group and the acid strength increases. Strong Acid/Strong Base  reaction between a strong acid and a strong base produces water and a salt  reaction goes until completion  resulting solution has neutral pH Strong Acid/Weak Base  pH of a solution resulting from the reaction of a strong acid with weak base is less than 7 (acidic) because of the presence of the conjugate acid of the weak base  proceeds to completion Strong Base/Weak Acid  of a solution resulting from the reaction of a strong acid with weak base is more than 7 (acidic) because of the presence of the conjugate acid of the weak base  proceeds to completion Weak Acid/Weak Base  the magnitude of the equilibrium constant and therefore the extent of reaction depend on the relative strength of the acids and bases in the reaction  equilibrium pH of the solution depends on the acid–base strength of the predominant species in solution


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