Chemistry 2e Chapter 14: pH, Acids & Definitions Guide

Arrhenius acid

when dissolved in water increase concentration of H3O+

Arrhenius base

when dissolved in water increases concentration of OH-

Bronsted-Lowry acid

proton donor (H+)

Bronsted-Lowry base

proton acceptor

Lewis acid

electron pair acceptor

Lewis base

electron pair donor

Conjugate acid-base pairs

-extension of Bronsted-Lowry theory

-net charge and mass must be the same on both sides

-acid-->conjugate base

-base-->conjugate acid

relative strengths

extend to which it ionized when dissolved in H2O

strong acid/base

complete ionization

weak acid/base

limited ionization

strong acids

HCl, HBr, HI, HNO3, H2SO4, HClO4

strong bases

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

pH

a quantitive way to express acidity

pOH

-log[OH-]

weak acids

react reversibly