chps 18 + 19 Flashcards by meagan b

strong acids

HCl
HNO3
H2SO4
HClO4
HBr
HI

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common acids

hydrochloric acid (HCl)
acetic acid (HC2H3O2)
sulfuric acid (H2SO4)
citric acid (HC6H7O4)
nitric acid (HNO3)
phosphoric acid (H4PO4)

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hydrochloric acid (HCl) use

steel industry

stomach acid

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acetic acid (HC2H3O2) use

vinegar

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sulfuric acid (H2SO4) use

batteries

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citric acid (HC6H7O4) use

citric fruits

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nitric acid (HNO3) use

fertilizers

explosive

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phosphoric acid (H4PO4) use

fertilizers

soft drinks

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common bases

ammonia (NH3)
sodium hydroxide (NaOH)
Ca(OH)2, Mg(OH)2, Al(OH)3

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ammonia (NH3) use

cleaner

fertilizer

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sodium hydroxide (NaOH) use

drain cleaner

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Ca(OH)2, Mg(OH)2, Al(OH)3 use

antiacids

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properties of acids

good conductors of electricity

corrosive (very reactive)

taste sour

react with metals to produce H2

react with bases to produce a salt and water

change the color of indicators

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properties of bases

good conductors of electricity

corrosive (very reactive)

taste bitter

feel slippery

react with acids to produce a salt and water

change the color of indicators

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acid: arrhenius traditional definition

a substance that dissolved in water to form H+ ions

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base: arrehenius traditional definition

a substance that dissolves in water to produce OH-

problem with arrehenius definitions of acid and base

definition require H2O- not all acids and bases are in H2O

acid: bronsted-dowry definition

a proton (H+) donor

base: bronsted-lowry definition

a proton acceptor

strong acids and bases

completely dissociate (separate into ions)

weak acids and bases

do not completely dissociate

what are the properties of acids and bases determined by?

how many ions are present

ampoteric

can act as an acid or a base (water)

weak acid (HA) dissociation equation

HA + H2O —> H3O+ + A-

dissociation constant (formula) Ka

Ka = ([H3O+][A-])/[HA]

weak base (B) dissociation equation

B + H2O —> OH- + HB+

dissociation constant (formula) Kb

Kb = ([OH-][HB+])/[B]

auto-ionization of water

2H2O — —> H3O+(aq) + OH-(aq) | Kw = [H3O+][OH-]

auto-ionization problems: determined if a solution is an acid, a base, or neutral

[H3O+]>[OH-] —> acid [H3O+] base [H3O+]=[OH-] —> neutral

salt

a compound consisting of the cation of a base and the anion of an acid salts can be acidic, basic, or neutral

titration

a procedure used to determine the concentration of an unknown acid or base