unit 10 Flashcards
general properties of acids
sour taste
able to dissolve many metals and neutralize bases
general properties of bases
bitter taste
slippery feel
ability to neutralize acids
Arrhenius definition of acid
a substance that produces H+ ions in solution
arrhenius definition of base
substance that produces OH- ions in solution
acids and bases combine to form
H2O and a salt
Bronsted-Lowry definition of Acids and Bases
acids (proton donors) and bases (proton acceptor s) always occur together in an acid-base reaction
conjugate acid-base pair
2 substances related to each other by the transfer of a proton
conjugate acid
any base to which a proton has been added
conjugate base
any acid from which a proton has been removed
strength of acids and bases proportion
inversely proportional
(stronger acid, weaker base and vice versa)
modern definition of acid
any compound having one or more hydrogen atoms that are weakly bound to the rest of the molecule. when dissolved in water, H+ ions ionize from the rest of the molecule.
what is the first element usually written in an acid compound?
H
what happens to organic acids when they ionize?
-COOH —-} -COO- + H+
amphoteric
capable of reacting as an acid or base
binary acids
contain H and one other atom
in aq solns, the name of every binary acid starts with _ and ends with _
hydro-, -ic
HF
hydrofluoric acid
HCl
hydrochloric acid
HBr
hydrobromic acid
HI
hydroiodic acid
H2S
hydrosulfuric acid
polyatomic anion acid rules
-ending of polyatomic anion name is changed, word acid is added
-if the polyatomic anion ends in -ate, it’s changed to -ic
-if the ending is -ite, its changed to -ous
sulfate changes to
sulfuric acid
sulfite changes to
sulfurous acid
nitrate changes to
nitric acid
nitrite changes to
nitrous acid
hypochlorite changes to
hypochlorous acid
chlorite changes to
chlorous acid
chlorate changes to
chloric acid
perchlorate changes to
perchloric acid
hydroxide bases
have hydroxide ions in their formulas, named using ionic compound nomenclature
NaOH name
sodium hydroxide
nitrogen bases definition
related to NH3 are amines
acid or base? HNO3
acid
acid or base? NH4+
acid
acid or base? KOH
base
acid or base? HC2H3O2
acid
strong acid
-equilibrium lies far to right
-acid ionizes completely
monoprotic acid
acids with only one ionizable proton
ex. HCl, HBr, HI
diprotic acid
acids with 2 ionizable protons
ex. H2SO4
weak acid
equilibrium lies far to left
-only small percentage of acid molecules ionize
nitric acid
HNO3
sulfuric acid
H2SO4
hydrofluoric acid
HF
acetic acid
HC2H3O2
sulfurous acid
H2SO3
carbonic acid
H2CO3
phosphoric acid
H3PO4
acid ionization constant
equilibrium constant for the ionization reaction of a weak acid
autoionization
water is amphoteric and can act as a base or acid with itself
autoionization reaction
H2O —-> H+ + OH-
ion product constant expression or dissociation constant (Kw)
ionization constant for water
[H3O+] x [OH-] = 1.0x10^-12
acidic solution
contains acid that increases [H3O+]
[OH-] decreases (= 1.0x10^-11 M)
[H3O+] > [OH-]
basic solution
contains a base that increases [OH-]
[H30+] decreases (= 1.-x10^-12 M)
[OH-] > [H3O+]
pH scale definition
specifies acidity of a solution
pH =
- log [H30+]
pH < 7
acidic
pH > 7
basic
pH = 7
neutral
change of 1 pH unit corresponds to
10-fold change in [H30+]
if the [H30+] has two sig figs, report answer to
2 decimal points
pOH scale definition
defined with respect to [OH-]
pOH =
- log [OH-]