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Definitions |
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1.00 x 10 ^ -14
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Kw = [H+][OH-] = ?
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Bronsted-Lowry acid
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A substance that can donate a proton
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sodium ethanoate
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Example of a buffer: ethanoic acid and ___________
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basic
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A weak acid titrated with strong base gives a(n) _____________ solution.
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NaOH, KOH, Ba(OH)2
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Three examples of strong bases
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aluminum, iron (III)
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Two examples of ions with a high charge density that form acidic salts
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Kw
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Ka x Kb = ?
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charge density
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Salts whose cation has a high ______________ will be acidic.
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acidic
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Strong acid titrated with weak base gives a(n) ______________ solution.
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neutralization
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Acids participate in _____________ reactions with bases.
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diprotic
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An acid is ____________ if it dissociates to give 2 mol of hydrogen ions in solution (for a strong one of these, [H+] will be twice the concentration of the acid).
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Bronsted-Lowry base
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A substance that can accept a proton
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size, charge
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The acidity of salts depends on the _________ and _________ of the cation.
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Lewis acid
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An electron pair acceptor
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[H+][A-]/[HA]
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For the dissociation of a weak acid (HA (aq) <----> H+ (aq) + A- (aq)), Ka = ?
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14
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pH + pOH = ?
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buffer
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A solution that resists changes in pH when a small amount of strong acid or strong base is added
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methyl orange
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Which indicator should be used for the titration of a strong acid with a weak base?
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[BH+][OH-]/[B]
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For the dissociation of a weak base, Kb = ?
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HCl, HNO3, H2SO4
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Three examples of strong acids
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14
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pKa + pKb = ?
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BH+ (aq) + OH- (aq)
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B (aq) + H2O (aq) <----> ?
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buffer region
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Part of a titration curve where the solution maintains the most constant pH (pKa = pH, the amount of base equal to half the amount required to reach equivalence has been added).
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Ka x ([HA]/[A-])
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The [H+] of a buffer solution = ?
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pH
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-log[H+]
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pKa
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The pH is equal to the _________ when the concentration of an acid and its conjugate base are equal.
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alkaline
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Salts made from a weak acid and strong base are ____________ in solution.
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H3O+ (aq) + A- (aq)
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HA (aq) + H2O (aq) <----> ?
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The dissociation of HA is minimal.
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What assumption is made in problems involving weak acid dissociation?
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NH3, amines
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Two examples of weak bases
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Lewis base
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An electron pair donor
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ammonium chloride
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Example of a buffer: ammonia and __________
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any
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Which indicator should be used for the titration of a strong acid with a strong base?
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red, yellow
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Methyl orange is _________ in acid and __________ in base.
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H2, salt
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Acids react with metals above hydrogen in the reactivity series to produce __________ and a ___________.
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CH3COOH, H2CO3
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Two examples of weak acids
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neutral
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Salts made from a strong acid and strong base are _____________ in solution.
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one half
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To prepare a buffer, combine a certain number of moles of a weak acid with ___________ the number of moles of a strong base.
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volumes, concentrations
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To prepare a buffer, combine equal ___________ of equal _____________ of an acid and its salt.
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indicator
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A weak acid or weak base whose salt is a different color; used in titrations
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increases
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The value of Kw _____________ as temperature increases.
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equivalence point
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In titrations, the name given to the point at which an equal number of moles of acid/base have been combined
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lower
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The weaker an acid is, the ___________ the value of the Ka is.
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neutral
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A strong acid titrated with strong base gives a(n) ______________ solution.
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HIn (aq)
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The symbol used to represent an indicator is _______.
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higher
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The weaker an acid is, the _____________ the pKa is.
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phenolphthalein
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Which indicator should be used for the titration of a weak acid with a strong base?
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acidic
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Salts made from a strong acid and weak base are _____________ in solution.
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colorless, pink
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Phenolphthalein is _________ in acid and __________ in base.
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equimolar
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A buffer consists of a weak acid or base and a(n) ______________ amount of its salt.
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equivalence point
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An indicator should be chosen with a pKa as close to the pH of the _____________ as possible (within one pH unit).
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CO2, H2O
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Acids react with carbonates and hydrogen carbonates to produce __________ and __________.
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