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Chemistry: Chpt 19

Acids and Bases

Acid more hydrogen ions than hydroxide ions
Base more hydroxide ions than hydrogen ions
pH the negative log of the hydrogen-ion concentration 0-7 = ACID 7-14 = BASE pH = -log[H+]
pOH the negative log of the hydroxide-ion concentration 0-7 = BASE 7-14 = ACID pOH = -log[OH-]
indicator acids or bases that undergo dissociation at a known pH
end point the point at which the indicator changes color
acid ionization constant Ka = (products/acid)
amphoteric substances that can act as both acids and bases
base ionization constant Kb = (products/base)
Arrhenius model
Bronsted-Lowry model Acid is the proton donor and the base is the proton acceptor
conjugate acid
Neutralization a base combined with an acid to neutralize an aqueous solution
weak acid/base ionize only slightly in an aqueous solution (acetic acid and ammonia)
strong acid/base completely ionized in an aqueous solution (HCl and NaOH)
salt combining OH- and H+ to make water and using whatever is left over to make a salt
standard solution
Properties of acids 1. sour taste 2. astringent feel on skin 3. turn blue litmus paper red 4. combine with base to form a salt 5. H3O+
Properties of Bases 1. taste bitter 2. feel slimy 3. turn red litmus paper blue 4. combine with acid to form a salt 5. OH-
Identify A/B Pairs 1. Determine which compounds go together 2. Loses an H+ (acid/con. base) 3. Gains an H+ (base/con. acid) TIPS (+) = acid (-) = base **acid/base always on left of yield **conj. A/B always on right of yield
Created by: simpsonsl15