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Acids
pH < 7 / pOH > 7
proton (H⁺) donors
acids are…
…compounds that release hydronium ions [H₃O⁺] when dissolved in water
-formula for most acids begin with H (ex: HCl)
acid effect indic: red
blue litmus & neutral litmus
acid effect indic: clear
Phenolphthalein
acid effect indic: no change
Red litmus
acids + active metals
produce H₂
acids + carbonates
produce H₂O + CO
net ionic equation
is about the formation of water
acids ionize
can be good electrolytes
Bases
pH > 7 / pOH < 7
proton (H⁺) acceptors
bases are…
… compounds that give off hydroxide ions [OH⁻] when dissolved in water
-formula for most bases ends with OH
bases dissociate
can be good electrolytes
amount / % / degree determines…
…the concentration of the solution
Neutralization reactions produce…
…salt (+ ion) and water (- ion)
Lewis acid
accepts electron pairs to form a covalent bond
Lewis base
donates electron pairs to form a covalent bond
Arrhenius acid
produces/increases hydronium [H₃O⁺] in water
Arrhenius base
produces/increases hydroxide [OH⁻] in water
Bronsted-Lowry acid
H⁺ proton donor
Bronsted-Lowry base
H⁺ proton acceptor
(BL) conjugate acid
the product of the BL base
(BL) conjugate base
the product of the BL acid
amphoteric
any substance that can act as an acid vice versa
Monoprotic acids
leading hydrogen is singular (ex: HCl)
can only donate one hydrogen proton
Diprotic acids
two leading hydrogen: H₂ (ex: H₂SO₄)
Triprotic acids
three leading hydrogren: H₃ (ex: H₃PO₄)
polyprotic acids
can donate >1 hydrogen protons
steps of ionization
if there are multiple hydrogren (polyprotic acids) the hydrogens will be given away in steps
Ionization Constant of Water
Kw = 1.0x10⁻¹⁴
K=[H₃O⁺] x [OH⁻]
1.0x10⁻¹⁴ = 1.0x10⁻⁷ x 1.0x10⁻⁷
H₃O⁺ and OH⁻ have an ______ relationship
inverse
log expression of acid concentration
pH = -log[H₃O⁺]
log expression of base concentration
pOH = -log[OH⁻]
pH / pOH
an expression of the concentration of an acid/base
titration
technique used to determine the concentration of an unknown acid or base by neutralizing it with a known acid or base
Neutralization
[H₃O⁺] = [OH⁻]
#H x M x V = #OH x M x V
equivalence point
the point at which neutralization occurs
end point
the point in a titration when the indicator changes colour
strong acids…
… ionize 100%
weak acids…
… ionize < 100%
strong bases…
… dissociate 100%
weak bases…
…dissociate < 100%
acids taste…
sour
bases taste __ and feel ___
bitter, slippery
carbonic acid: H₂CO₃
formed when an acid interacts with a carbonate
H₂O and CO₂
formed when carbonic acid (H₂CO₃) continues to break down
Note 
Flashcard (116)