ACIDS AND BASES
ACIDS
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Release H+ ions in aqueous solution (Arrhenius theory)
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Can accept a pair of electrons (Lewis theory)
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Can donate a proton (Bronsted-Lowry theory)
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Taste sour or tart
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Aqueous solutions are electrolytes
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(strong acid = strong electrolyte) ​
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BASES
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Release OH- ions in aqueous solution (Arrhenius theory)
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Can donate a pair of electrons (Lewis theory)
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Can accept a proton (Bronsted-Lowry theory)
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Bitter taste and feel slippery
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Soluble bases are alkalis
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Aqueous solutions are electrolytes
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(strong base = strong electrolyte)​
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The acid and base in a conjugate pair differ by one proton!
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- Strong acids have weak conjugate bases.
- Weak acids have strong conjugate bases.
Amphiprotic - In terms of protons; can act as either a proton donor or acceptor. All amphiprotic species are amphoteric (can act as a base or acid).
e.g.
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HCO3- (hydrogen carbonate ion)
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HSO4- (hydrogen sulfate ion)
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H2PO4- (dihydrogen phosphate ion)
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HPO4 2- (hydrogen phosphate ion)
THE STRENGTH OF AN ACID/BASE
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CONDUCTIVITY
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pH
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RATE OF REACTION
A salt can be:
NEUTRAL (strong acid + strong base)
BASIC (weak acid + strong base)
ACIDIC (strong acid + weak base)
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cation from base + anion from acid = salt
CONCENTRATION - Amount of solute dissolved in per unit volume of solvent.
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STRENGTH - Extent to which an acid or a base can get ionized when dissolved in water.
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*Strong acid is a good proton donor and has a weak conjugate base (equilibrium lies to far right)
*Weak acid is not a good proton donor but has a strong conjugate base (equilibrium lies to far left)
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HCl - Hydrochloric acid
HBr - Hydrobromic acid
HI - Hydroiodic acid
HClO4 - Perchlorate acid
H2SO4 - Sulfuric acid
HNO3 - Nitric acid
