Gen Chem-Acids and Bases

properties of acids

taste sour, dissolve many metals, turn blue litmus paper red, neutralize bases

properties of bases

taste bitter, feel slippery, turn red litmus paper to blue, neutralize acids

Arrhenius acid

any substance that produces H+ ions in an aqueous solution

Arrhenius base

any substance that produces OH- ions in an aqueous solution

Bronsted-Lowry Acid

proton (H+) donor

Bronsted-Lowry Base

proton (H+) acceptor

Lewis acid

e- pair donor

Lewis base

e- pair acceptor

conjugate acid

a base to which a H+ has been added

conjugate base

an acid to which a H+ has been removed

strong acids

HCl, HBr, HI, HNO3, H2SO4, HClO4

strong acid properties

completely dissociates in solution, equilibrium falls to the right

Ka value affect on acid strength

smaller k value means it’s a weaker acid

weak acid properties

partially dissociates in solution, equilibrium falls to the left

autoionization

chemical reaction between 2 molecules of the same substance to produce ions

pH

\-log(\[H+\])

pOH

\-log(\[OH-\])

pKa

\-log(Ka)

lower the pKa

stronger the acid

ph below 7

acidic

ph above 7

basic

ph at 7

neutral

WA w/ WA

ignore all but the strongest of the weak acids

ph + pOh=

14

SA w/ WA

\[H+\] in ICE table is from the strong acid

polyphonic acid

typically ionizes in successive steps with its own Ka

Ka

equilibrium constant of an acid

Kb

equilibrium constant of a base

Kw

equilibrium constant of water

value of Kw

1\.00 x 10^-14

amphoteric

can act as an acid or a base

anions

form base or neutral solution

cations

form acidic or neutral solution

anion of a CB of a weak acid

is a weak base

anion of a CB of a strong acid

is pH neutral

Kw=

(Ka)(Kb)jo

counter ions of SB

pH neutral

cations that are conjugates acids of a WB

are acidic

small highly charged metals

form weakly acidic substance except group I, II metals

ph of salt solution

depends on both cations and anions

salt with both cation and anions

are pH neutral

salts where cation is neutral but anion is basic

are basic

salts were cation is acidic but anion is neutral

are acidic

salts where cation is acidic but anions is basic

depends on relative strength of each ion

Ka>Kb

acidic

Kb>Ka

basic\`

binary acids

H w/ one other element

binary acid strength

depends on bond polarity and bond strength( more polar, more acidic)(stronger bond, less acidic)

oxyacids

H bonded to an O which is bonded to another element

oxyacid strength

depends on EN of other element and number of oxygens