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CHEMISTRY: FOUNDATION REVIEW > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

Defined an acid as a species that donates H+ (protons) in an aqueous sol’n and a base as a species that produces OH- (hydroxide ions) in an aqueous sol’n

A

Arrhenius

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2
Q

any species that donates protons

*Do not necessarily have to dissociate into H+ in aqueous sol’n

A

Bronsted-Lowry acid

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3
Q

any species that accepts protons
*Do not necessarily have to dissociate to form OH- in aqueous sol’n
(Ex: NH3 and Cl-)

A

Bronsted-Lowry base

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4
Q

Defines a ______ as an electron-pair acceptor

A

Lewis acid

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5
Q

defines a _____ as an electron-pair donor

A

lewis base

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6
Q

Bronsted-Lowry acids and bases always occur in pairs, called _______. The two members are related by the transfer of a proton

A

conjugate acid-base pairs

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7
Q

The stronger the acid, the _______ its conjugate base

A

weaker

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8
Q

the weaker the acid, the ________ its conjugate base

A

stronger

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9
Q

H2O can act as either a ________ or a _____ with other species or with itself
H2O + H2) —-> H3O+ + OH-

A

proton donor or acceptor

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10
Q

Constant that describes _______, or acting as a proton donor/acceptor toward itself

A

Autoionization: Kw

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11
Q

Equation: Kw (Autoionization constant)

A

Keq = Kw = [H3O+][OH-]

Note: Kw for water = 110^-14

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12
Q

measures hydrogen ion (proton) concentration

pX = -log(X) where [H+] is its molarity and the logarithm is of base 10

A

pH

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13
Q

Equation: pH

A

pH = -log[H+] = log (1/[H+])

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14
Q

The power to which 10 would be raised to obtain the number x

A

Log(x)

i.e. [H+] = 1 * 10^-3 then pH = 3

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15
Q

have a pH less than 7
relative excess of H+ ions
Ex: Lemon juice, gastric juice

A

acidic sol’n

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16
Q

pH greater than 7
relative excess of OH- ions
Ex: baking soda, bleach, ammonia

A

basic sol’n

17
Q

pH = 7

Ex: water

A

neutral sol’n

18
Q

completely dissociate into their component ions in aqueous sol’n

A

strong acid and bases

19
Q

Examples of this include: HClO4, HNO3, H2SO4, HCl, HBr, HI

A

strong acids

20
Q

Examples of this include: NaOH, KOH, soluble hydroxides of Group IA and IIA metals

A

strong bases

21
Q

substances that do not ionize completely (only partially)

weak electrolytes

A

weak acids and bases

22
Q

equilibrium constant for acid ionization
acid dissociation constant
measure of the degree to which an acid dissociates
smaller for weaker acids

A

Ka

23
Q

equilibrium constant for base ionization

A

Kb

24
Q

the smaller the _____, the weaker the acid (i.e. must smaller than 1)

A

Ka

25
Q

Equation: Ka

A

Ka = [H+][A-] / [HA]

Note: [A-] = conjugate base; [HA] = weak acid

26
Q

Strategy: Calculate the pH for sol’ns of weak acids

A
  1. ID start concentration for weak acid (reactant) and H+ and A- (product)
  2. Calculate change in concentration
  3. ID end concentration of weak acid (reactant) and H+ and A-
27
Q

The concentratino of teh weak acid at equilibrium = it’s initial concentration minus the _______

A

amount dissociated

28
Q

The concentration of [H+] dissociated from a weak acid equals ______

A

amount of conjugate base formed

29
Q

the addition of a sol’n of known concentration and volume to another sol’n to determine its unknown concentrations
involved the addition of a sol’n to determine its concentration

A

titrations

30
Q

add base of precisely known concentration drop by drop to an acid solution until the numbero f moles of base added equals the number of moles of acid initially present

A

acid-base titration

31
Q

point at which the number of moles of base added equals the number of moles of acid initially present in an acid-base titration

A

equivalence point

32
Q

Equation: Acid-Base titration at equilibrium point

A

Va * Ma = Vb * Mb
Note: Va = initial volume of acid solution; Ma = acid’s molarity (trying to determine); Vb = volume of base added; Mb = molarity of the base (known precisely before)

33
Q

T/F: The equivalence point in an acid-base titration must occur at pH 7

A

False

34
Q

Titrations between a strong acid and strong base have an equivalence point at pH =

A

7

35
Q

titration between a weak acid and a strong base has an equivalence point at pH ______

A

> 7

CHEMISTRY: FOUNDATION REVIEW (9 decks)

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