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CHEM 14203 > LO 42 - 46 > Flashcards

LO 42 - 46 Flashcards

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1
Q

What is a neutralization reaction?

A

acids react with bases and produce H2O or sometimes a weak electrolyte

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2
Q

Weak acids do not _________ so they are notated by ↔ reaction arrows

A

fully ionize

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3
Q

________ acids contain more than one ionizable proton and release them _________

A

polyprotic
sequentially

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4
Q

_______ acids have one, first strongly ionizable proton and then a second weaker one

A

diprotic

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5
Q

________ acids contain only two elements

A

binary

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6
Q

How are binary acids named?

A

hydro + base name of nonmetal (-ic) + acid

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7
Q

________ contain H and an oxyanion which is a nonmetal + oxygen

A

oxyacid

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8
Q

How are oxyacids named when the oxyanion ends in -ate?

A

base name of oxyanion + -ic + acid

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9
Q

How are oxyacids named when the oxyanion ends in -ite?

A

base name of oxyanion + -ous + acid

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10
Q

Describe acid-base titrations

A

a substance in solution of known concentration is reacted with another solution of unknown concentration. an indicator such as dye is used to signal the equivalence point

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11
Q

What is the titration equivalence point

A

when the # of mols OH- equals the number of mols H+ in solution

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12
Q

Neutralization reactions between concentrated acids and bases are highly __________

A

exothermic

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13
Q

What are the 4 distinct characteristics of acids

A
  1. sour taste
  2. dissolve many metals
  3. turn litmas paper blue → red
  4. neutralize bases
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14
Q

What are the four distinct characteristics of bases

A
  1. bitter taste
  2. slippery feeling
  3. turn litmas paper red → blue
  4. neutralize acids
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15
Q

What is the Arrhenius definition of an acid

A

a substance that produces H+ ions in aqueous solution

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16
Q

What is the Arrhenius definition of a base

A

a substance that produces OH- ions in aqueous solution

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17
Q

Weakness or strength of an acid/base is determined by __________ according to Arrhenius

A

amount that dissociates into ions

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18
Q

What is the Bronsted-Lowry definition of an acid

A

a proton donor

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19
Q

What is the Bronsted-Lowry definition of a base

A

a proton acceptor

20
Q

__________ substances such as H2O can act as an acid or a base

A

amphoteric

21
Q

____________ acid-base pairs are two substances related to each other by the transfer of a proton

A

conjugate

22
Q

Base + H+ → ______

A

conjugate acid

23
Q

Acid - H+ → ________

A

conjugate base

24
Q

What two factors affect the strength of a binary acid

A
  1. bond polarity
  2. bond strength
25
Q

How does bond polarity impact the strength of a binary acid

A

Increasing the polarity of an “H-X” bond increases the strength of the acid. When shared electrons in an “H-X” bond spend most of their time close to “X” atom, the bond becomes polar. It also becomes weaker.

26
Q

How does bond strength impact the strength of binary acids

A

the stronger the bond the weaker the acid because the H atom will be held more tightly

27
Q

What two factors affect the strength of an oxyacid (HYOx)

A
  1. electronegativity of “Y”
  2. number of oxygens bonded to “Y”
28
Q

How does the electronegativity of “Y” in an oxyacid (HYOx) impact strength of the acid

A

the more electronegative Y, the more it weakens and polarizes the H-O bond and thus the more acidic

29
Q

How does the number of oxygens bonded to “Y” in an oxyacid (HYOx) impact strength of the acid

A

additional O atoms are electronegative and thus draw e- density away from the bonds to Y and H, weaking the bonds and increasing acidity

30
Q

The ______ ________ constant (Ka) quantifies the relative strength of a weak acid based on the law of mass action

A

acid ionization

31
Q

The smaller Ka is, the _______ the acid ionizes thus indicating it as _______

A

less
weaker

32
Q

Because water is amphoteric, it acts as an acid or base with itself in a process known as ________

A

autoionization

33
Q

The ______________ of water (Kw) represents H2O at equilibrium

A

ion product constant

34
Q

Kw = ____________ (concentration terms) @ 25°C

A

[H3O+] · [OH-]

35
Q

Kw = ____________ (numeric) @ 25°C

A

1.0 · 10^-14

36
Q

A neutral solution contains
[H3O+] = [OH-] = ____________ @ 25°C

A

1.0 · 10^-14

37
Q

An acidic solution contains
[H3O+] _____ [OH-]

A

>

38
Q

A basic solution contains
[H3O+] _____ [OH-]

A

<

39
Q

In aqueous solutions both [H3O+] and [OH-] are present and _________ holds true

A

[H3O+] · [OH-] = 1.0 · 10^-14

40
Q

A “p” scale of any kind indicates the _________ of a value

A

-log (x)

41
Q

The pH scale specifics the _______ of a solution as given by pH = _______

A

acidity
-log [H3O+]

42
Q

pH + pOH = ______

A

14

43
Q

The numbers to the right of the decimal place in a pH or pOH value correspond to the number of ________________

A

significant figures in the negative log
ex. -log (1.0 · 10^-3) = 3.00 pH
2 sig figs 2 decimal places

44
Q

pKa = _________ where the smaller the pKa value, the _________ the associated acid

A

-log(Ka)
stronger

45
Q

For oxyacids (H-X-O):
more electronegative X = _________
more O atoms = ___________

A

stronger,
stronger

46
Q

For binary acids (H-A):
larger the atom = ____________

A

stronger

47
Q

Strong acids and strong bases do not ____________________. As such, when you get the conjugates of a SA or SB in the products side of a reaction . . .

A

reform in solution
they will be neutral

CHEM 14203 (21 decks)

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