Gen. Chem ch 14: acid/base theory

sour

taste of aqueous solutions of acids

red

an acid on litmus paper

clear

an acid with phenolphthalein

hydrogen gas

produced when some acids react with active metals

salts and water (neutralization reaction)

produced when acids react with bases

strong acid

dissociates 100% in water

weak acid

only partly dissociates in water

electrolytes

acids and bases are both

bitter

taste of aqueous solutions of bases

blue

a base on litmus paper

pink/purple

a base with phenolphthalein

soapy/slippery

base solutions feel ___

Arrhenius Acid

a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution (starts with H+)

Arrhenius Base

a chemical compound that increases the concentration of hydroxide ions, OH-, in aqueous solutions (ends with OH-)

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

7 strong acids

H2SO4

only the first hydrogen is a strong acid

base strength

the strength at which a base ionizes/dissociates

acid strength

the strength at which an acid ionizes/dissociates

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

7 strong bases

Bronsted-Lowry acid

a molecule or ion that is a proton (H+) donor (proton H+ producer)

Bronsted-Lowry base

a molecule or ion that is a proton acceptor (proton H+ acceptor)

Bronsted-Lowry Acid-Base Reaction

when a proton is transferred from one reactant to another (acid to base)

Monoprotic Acid

an acid that can only donate one proton per molecule

Polyprotic Acid

an acid that can donate more than one proton per molecule

Diprotic acid

can donate 2 protons per molecule

Triprotic acid

can donate 3 protons per molecule

Lewis Acid

an atom, ion, or molecule that accepts an electron pair to form a covalent bond (electron-pair acceptor)

Lewis Base

an atom, ion, or molecule that donates an electron pair to form a covalent bond (electron-pair donor)

Lewis Acid-Base Reaction

the transfer of one set of electrons between the acid and base to form a covalent bond

H2O

not Arrhenius

Conjugate Base

the species that remains after a Bronsted-Lowry acid has given up a proton (BA > CB)

Conjugate Acid

the species that is formed when a Bronsted-Lowry base accepts a proton (BB > CA)

relative strengths of the acids and bases involved

What does the extent of the reaction between a Bronsted-Lowry acid and base depend on?

the weaker its conjugate base

the stronger the acid…

the weaker its conjugate acid

the stronger the base…

sulfur

main component that causes acid rain

hydrogen power

pH stands for the French words pouvoir hydrogene, meaning __

pH

a solution is defined as the negative of the common logarithm of the hydronium ion concentration

-log[H3O+]

pH =

pOH

a solution is defined as the negative of the common logarithm of the hydroxide ion concentration

basic

pH greater than 7

acidic

pH less than 7

7

neutral

basic

pOH less than 7

acidic

pOH greater than 7

-log[OH-]

pOH =