Acids and Bases
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Last updated 6:37 PM on 5/4/23
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46 Terms
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Acids
pH < 7 / pOH > 7
proton (H⁺) donors
proton (H⁺) donors
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acids are…
…compounds that release hydronium ions \[H₃O⁺\] when dissolved in water
\-formula for most acids begin with H (ex: HCl)
\-formula for most acids begin with H (ex: HCl)
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acid effect indic: red
blue litmus & neutral litmus
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acid effect indic: clear
Phenolphthalein
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acid effect indic: no change
Red litmus
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acids + active metals
produce H₂
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acids + carbonates
produce H₂O + CO
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net ionic equation
is about the formation of water
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acids ionize
can be good electrolytes
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Bases
pH > 7 / pOH < 7
proton (H⁺) acceptors
proton (H⁺) acceptors
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bases are…
… compounds that give off hydroxide ions \[OH⁻\] when dissolved in water
\-formula for most bases ends with OH
\-formula for most bases ends with OH
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bases dissociate
can be good electrolytes
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amount / % / degree determines…
…the concentration of the solution
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Neutralization reactions produce…
…salt (+ ion) and water (- ion)
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Lewis acid
accepts electron pairs to form a covalent bond
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Lewis base
donates electron pairs to form a covalent bond
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Arrhenius acid
produces/increases hydronium \[H₃O⁺\] in water
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Arrhenius base
produces/increases hydroxide \[OH⁻\] in water
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Bronsted-Lowry acid
H⁺ proton donor
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Bronsted-Lowry base
H⁺ proton acceptor
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(BL) conjugate acid
the product of the BL base
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(BL) conjugate base
the product of the BL acid
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amphoteric
any substance that can act as an acid vice versa
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Monoprotic acids
leading hydrogen is singular (ex: HCl)
can only donate one hydrogen proton
can only donate one hydrogen proton
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Diprotic acids
two leading hydrogen: H₂ (ex: H₂SO₄)
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Triprotic acids
three leading hydrogren: H₃ (ex: H₃PO₄)
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polyprotic acids
can donate >1 hydrogen protons
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steps of ionization
if there are multiple hydrogren (polyprotic acids) the hydrogens will be given away in steps
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Ionization Constant of Water
Kw = 1.0x10⁻¹⁴
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K=\[H₃O⁺\] x \[OH⁻\]
1\.0x10⁻¹⁴ = 1.0x10⁻⁷ x 1.0x10⁻⁷
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H₃O⁺ and OH⁻ have an ______ relationship
inverse
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log expression of acid concentration
pH = -log\[H₃O⁺\]
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log expression of base concentration
pOH = -log\[OH⁻\]
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pH / pOH
an expression of the concentration of an acid/base
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titration
technique used to determine the concentration of an unknown acid or base by neutralizing it with a known acid or base
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Neutralization
\[H₃O⁺\] = \[OH⁻\]
\#H x M x V = #OH x M x V
\#H x M x V = #OH x M x V
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equivalence point
the point at which neutralization occurs
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end point
the point in a titration when the indicator changes colour
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strong acids…
… ionize 100%
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weak acids…
… ionize < 100%
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strong bases…
… dissociate 100%
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weak bases…
…dissociate < 100%
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acids taste…
sour
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bases taste __ and feel ___
bitter, slippery
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carbonic acid: H₂CO₃
formed when an acid interacts with a carbonate
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H₂O and CO₂
formed when carbonic acid (H₂CO₃) continues to break down
