chem acid & bases

acid

a compound that ionizes to form hydrogen or hydronium ions in water

base

a compound that ionizes to form Hydroxide (OH-)ions in water

tastes sour

acids

feels slippery

bases

conducts electricity

both

hydrogen acceptor

bases

tastes bitter

bases

litmus paper. red—>blue

bases

bromothymol blue turns yellow

acids

phenolphthalein turn clear (colorless)

acids

phenolphthalein turns pink

bases

bromothymol blue turns blue

bases

feels watery

acids

hydrogen donor

acids

corrosivity: strong/most

acids

litmus paper: blue —> red

acids

corrosivity: strong

bases

H+ or H3O+ ions produced

acids

OH- ions

bases

white vinegar

acids

lemon juice

acid

bleach

bases

soap

bases

lye (drain cleaning)

bases

soda

acids

strong acid/base

completely dissociates(breaks apart)

weak acid/base

slightly dissociates

HCl

strong acid

LiOH

strong base

NaOH

strong base

RbOH

strong base

HBr

strong acid

CsOH

strong base

HI

strong acid

HNO3

strong acid

KOH

strong base

Ca(OH)2

strong base

Sr(OH)2

strong base

HClO4

Strong acid

HClO3

strong acid

Br(OH)2

strong base

H2SO4

strong acid

strong acids (7)

HCl, HBr, HI, HNO3, HClO4, HClO3, H2SO4

strong bases (8)

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

strong bases are located in

group 1 (not H) and group 2

the lower the PH the ____ acidic

stronger

the lower the PH level the ______ basic

weaker

the higher the PH level the _____ acidic

weaker

the higher the PJ level the _____ basic

stronger

above 7

base

below 7

acid

exactly 7

neutral

Bronsted-Lowry Acids

Compounds that donate protons (H+) to a base

Bronsted-Lowry bases

compounds that accept protons (H+) from an acid.

conjugate base

formed when an acid donates a proton. It can react with a proton to form the original acid.

conjugate acid

formed when a base accepts a proton. It can donate a proton to form the original base.

Lewis acids

substances that accept an electron pair from a base

lewis bases

substances that donate an electron pair to a Lewis acid.

arrhenius acids

increases the concentration of hydrogen (H+) or hydronium(H3O+)

Arrhenius bases

increases the concentration of hydroxide (OH-)