Skip to main content
Back

223z_midterm1

Control buttons has been changed to "navigation" mode.
1/74
  • list of strong acids (6)


    HNO3 < H2SO4 < HCl < HBr < HI < HCLO4

  • list of strong bases (6)


    LiOH < NaOH < KOH < Sr(OH)2 < Ca(OH)2 < Ba(OH)2

  • (๐›‚) more stable base resonance structure


    (๐›‚) stronger acid

  • (๐›ƒ) larger atoms (down a group)


    (๐›ƒ) stronger acid

  • (๐›„) electronegative surroundings


    (๐›„) stronger acid

  • group 2 hydroxide


    release 2 OH-, more base per mole

  • larger ions


    separate more easily

  • more soluble


    stronger base

  • arrhenius acid


    substance that produces H+ ions

  • arrhenius base


    substance that produces OH- ions

  • electrolyte (acid/base)


    substance that forms ions in solution

  • electrolyte strength


    depends on extent of dissociation

  • strong acid/base


    complete dissociation

  • weak acid/base


    partial dissociation

  • brรธnsted-lowry acid


    proton (H+) donor

  • brรธnsted-lowry base


    proton (H+) acceptor

  • amphoteric substance


    can act as an acid or a base

  • conjugate acid-base pair


    2 substances related by the transfer of a proton

  • conjugate acid


    a base with a proton added to it

  • conjugate base


    an acid with a proton removed from it

  • binary acid


    H-Y

  • oxyacids


    H-O-Y

  • acidic H-Y bond


    H atom has positive dipole moment

  • increasing acidity


    decreasing bond strength

  • factors (2) affecting H-O-Y strength


    electronegativity of Y, number of O atoms bonded to Y

  • far right equilibrium


    complete ionization

  • monoprotic acid


    only 1 ionizable proton

  • hydrofluoric acid


    HF (weak)

  • acetic acid


    HC2H3O2 (weak)

  • formic acid


    HCHO2 (weak)

  • sulfurous acid


    H2SO3 (weak)

  • carbonic acid


    H2CO3 (weak)

  • phosphoric acid


    H3PO4 (weak)

  • acid ionization constant (Ka)


    quantifies acid strength

  • smaller Ka


    less ionization in water

  • pKa


    -log(Ka)

  • autoionization


    water acts as an acid/base with itself

  • ion product constant (Kw)


    [H3O+] x [OH-] = 1.0 x 10^-14

  • acidic solution


    [H3O+] > [OH-]

  • basic solution


    [H3O+] < [OH-]

  • pH


    -log[H3O+]

  • pH scale [H+]


    decreases by a factor of 10

  • smaller pKa


    stronger acid

  • Ka


    [HA] [A-] / [HA]

  • % ionization of a weak acid


    [H3O+] at equilibrium divided by initial [HA]

  • with increasing [HA]initial


    [H3O+]eq increases, % ionization decreases

  • [H3O+] for a mix of acids


    [strong acid] = total [H3O+]

  • most weak bases


    act as a base by accepting a proton from water

  • most strong bases


    group 1A and 2A metal hydroxides

  • group 2A: M(OH)2


    dissociates in a single step

  • amines (most weak bases)


    ammonia with 1+ hydrocarbon groups substituted for 1+ hydrogen atoms, have a nitrogen atom w/ a lone pair acting as a proton acceptor

  • anions


    form basic or neutral solutions

  • cations


    form acidic or neutral solutions

  • anion that's a conj. base of a weak acid


    weak base

  • anion that's a conj. base of a strong acid


    pH neutral

  • Kb of an anion


    use Ka of its conj. acid

  • (cation) counterions of strong bases


    pH neutral

  • (cation) conj. acids of weak bases


    weakly acidic

  • (cation) small highly charged metals


    weakly acidic

  • (salts) cation/anion doesn't act as an acid/base


    neutral solution

  • (salts) anion acts as a base


    basic solution

  • (salts) cation acts as an acid


    acidic solution

  • (salts) cation/anion acts as an acid/base


    ion with the higher K determines pH

  • polyprotic acids


    ionizes in successive steps, Ka1 > Ka2

  • lewis acid


    electron pair acceptor (has an incomplete octet)

  • lewis base


    electron pair donor

  • adduct


    product of a lewis acid/base reaction

  • conj. acid of a weak base (low tendency to accept protons)


    high tendency to donate protons

  • hydrolysis


    ion reacts with water to form H+ or OH-

  • conj. base of a weak acid


    produces OH-

  • conj. acid of a weak base


    produces H3O+

  • small, highly charged metal cations


    produces H3O+

  • conjugates of strong acids


    neutral pH

  • conjugates of strong bases


    neutral pH