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Chem > Chapter 9; Acids and Bases, pH, and Buffers > Flashcards

Chapter 9; Acids and Bases, pH, and Buffers Flashcards

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1
Q

what is acid base homeostasis range

A

7.35 - 7.45
proper organ function requires blood pH

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2
Q

what is the range of blood pH for it to be acidosis

A

pH < 7.35

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3
Q

what is the range of blood pH for it to be alkalosis

A

pH > 7.45

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4
Q

what is the blood pH ranges

A

6.6 - 8.0

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5
Q

what do acids produce in aqueous solutions

A

hydronium ions, H subscript 3 O+ ; H3O+

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6
Q

what do bases produce in aqueous solutions

A

hydroxide ions, OH-

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7
Q

according to the Arrhenius definition what are the two conditions

A
  • an acid is a substance that produces hydronium ions, H3O+
  • and a base is a substance that produces hydroxide ions, OH-, in aqueous solution
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8
Q

what are group 1A hydroxide salts in ionic compounds containing hydroxide ions being bases

A

NaOH, KOH
soluble in water
strong electrolytes
dissolve entirely to produce ions in water

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9
Q

what are 2A hydroxide salts in ionic compounds containing hydroxide ions being bases

A

Ca(OH)2, Mg(OH)2
slightly soluble in water
weak electrolytes (not many ions)
dissolve slightly to produce few ions in water

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10
Q

ionic compounds composed of hydroxide ion (OH-) are bases because they produce

A

solvated hydroxide ions in solution

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11
Q

are soluble hydroxide ion salts (group 1A salts strong or weak electrolytes

A

strong

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12
Q

are slightly soluble hydroxide ion salts (group 2A salts) strong or weak electrolytes

A

weak

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13
Q

in the Bronsted-Lowry theory of acids and bases, how are an acid and base differentiated

A

acid: a proton (H+) donor
base: a proton (H+) acceptor

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14
Q

in bronsted lowry theory what is the term of neutral acid loses proton to form

A

conjugate base
(one fewer H+ and, a -1 charge; compared to formula of acid

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15
Q

in bronsted Lowry theory what is the term when water acts as a base, accepting proton to form

A

conjugate acid
(one more H+, a +1 charge; compared to formula of base)

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16
Q

what does a base combine with to produce its conjugate acid

A

H+
base + H+ (<-,->) conjugate acid

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17
Q

according to the Bronsted Lowry theory, can water accept and/or donate a proton

A

can accept or donate

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18
Q

can water act as an acid or a base according to the bronsted Lowry theory

A

both

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19
Q

what is the term under the bronsted Lowry theory for any substance that can act as an acid or a base

A

amphoteric compound

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20
Q

in a conjugate acid-base pair; an acid and its conjugate base or a base and its conjugate acid are called a conjugate acid-base pair

A

yes

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21
Q

can all H+ be donated

A

usually indicated at the beginning of the formula
e.g
HCl -> Cl- chloride ion
HC2H3O2 -> C2H3O2- acetate ion

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22
Q

the strength of an acid depends on the ….

A

extent to which the acid donates a proton to water

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23
Q

the strength of a base depends on the extent to which…

A

the base accepts a proton from water

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23
Q

strong acids dissociate in water […] to form a conjugate base and hydronium ions

A

completely

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24
Q

is HCl really strong

A

yes, the only strong acid produced in the human body

25
Q

strong acids are highly […] when concentrated but are safe to handle as […] solutions

A

corrosive
dilute

26
Q

what are the common strong acids

A

HNO3
H2SO4
HCLO4
HCL
HBr
HI

27
Q

in a solution, what does the strong acid contain mostly and very little of

A

mostly H3O+ and the conjugate base, and very little of the acid

28
Q

why are strong acids strong electrolytes

A

base they produce many ions in solution

29
Q

what groups make up strong bases

A

1A and 2A metal ions with hydroxide ions

30
Q

do strong bases (groups 1A and 2A) completely dissociate in aqueous solutions

A

yes, producing hydroxide ions and cations (conjugate acids)

31
Q

are strong bases (1A and 2A) strong electrolytes

A

if soluble

32
Q

strong bases (1A and 2A) are […] corrosive when concentrated; can be handled safely as […] solutions

A

highly
dilute

33
Q

what are common strong bases

A

Ba(OH)2
Ca(OH)2
LiOH
KOH
NaOH
Sr(OH)2
appear to contain OH

34
Q

strong acids […] ionize, where weak acids only […] ionize

A

completely
partially

35
Q

a weak acid, and similarly a weak base, undergo a reversible reaction with water that, at equilibrium, favors the […]

A

reactants

36
Q

what are e.g. of weak acids

A

CH3COOH
H3PO4
H2CO3
any acid not listed in the six common strong acids

37
Q

what are some weak bases

A

NH3
CH3NH2

38
Q

what is Le Chatelier’s principle

A

reaction shifts in direction that counteracts a disturbance
- forward reaction enhanced (a shift to the right) until a new equilibrium is attained)
- reverse reaction enhanced (a shift to the left) until a new equilibrium is attained

39
Q

what is Le CHatelier’s principle important in reactions

A

weak acid and weak base reactions

40
Q

what are biochemical pathways in Le Chatelier’s principle

A

reactions are approaching equilibrium

41
Q

how to identify a weak strong or non electrolyte through pictures

A

weak; some + and - charges while others have no indication of charge
strong; equal number of + and - charged particles
non; no indication at all of charges

42
Q

what does pH measure

A

concentration of hydronium ions (H3O+) in aqueous solution

43
Q

H3O+ = molar concentration (mole/L) of

A

H3O+

44
Q

OH- = molar concentration of

A

OH-

45
Q

pH < 7 is

A

acidic
[H3O+] > [OH-]
brackets indicate concentration of hydronium ions

46
Q

pH > 7 is

A

basic (alkaline)
[H3O+] < [OH-]
brackets indicate concentration of hyronium ions

47
Q

PH = 7 is

A

neutral
[H3O+] = [OH-]
brackets indicate concentration of hydronium ions

48
Q

what is auto ionization of water

A

occurs when very few water molecules react with other water molecules to produce hydronium ions and hydroxide ions

49
Q

in pure water at 25 degrees celsius what is the power of 10 for M in H3O+

A

1.0 x 10^-7 M

50
Q

In pure water at 25 degrees celsius what is the power of 10 in M for OH-

A

1.0 x 10^-7 M

51
Q

what is the power of 10 for K subscript w Kw

A

Kw = 10^-14
which is
Kw = [H3O+] x [OH-]

52
Q

Kw is

A

ion product constant for water

53
Q

when acid or base is added to water, auto ionization of water shifts, but Kw is

A

constant. Kw = 10^-14

54
Q

when hydronium ion […], hydroxide must […]

A

increase
decrease

55
Q

when adding acid to water; what does [H3O+] increases from 1x10^-7 M to

A

1x10^-6 M

56
Q

how to calculate the pH from the hydronium ion concentration

A

pH = -log subscript 10 [H3O+]
for pure water,
pH = -log subscript 10 [1x10^-7]

57
Q

when calculating pH from the hydronium ion concentration what is pH of an aqueous solution

A

the logarithm of the hydronium ion concentration multiplied by -1

58
Q

to find the [OH-] hydroxide ion concentration the equation is

A

pH + pOH = 14

59
Q

the more hydronium ions [H3O+] the more the solution is

A

acidic

60
Q

the more hydroxide ions [OH-} the more the solution is

A

basic

Chem (9 decks)

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