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BIOCHEM LAB > EXERCISE 1 - 2 > Flashcards

EXERCISE 1 - 2 Flashcards

1
Q
  • almost all processes containing ____ have a need for pH measurement
A

WATER

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2
Q

compares the acidity or alkalinity of a solution at a given temperature

A

pH

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3
Q

neutral pH

A

pH 7

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4
Q

pH can only be measured if it is in ____ form

A

AQUEOUS

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5
Q

pH measures the dami ng

A

H+

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6
Q

neutral solution activity

A

H & OH are equal

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7
Q

acidic

A

ph < 7

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8
Q

acidic soln activity

A

H activity ↑ ; pH value ↓

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9
Q

basic

A

pH > 7

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10
Q

basic soln activity

A

OH activity ↑ ; pH value ↑

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11
Q

H activity and pH is

A

inversely proportional

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12
Q

the acidity and basicity of a substance can be measured in terms of

A

MOLAR CONCENTRATION

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13
Q

to provide ease in expressing these values, the concentration and OH- ions are denoted as

A

pH and pOH

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14
Q

the pH of a solution may be measured using

A

pH paper

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15
Q

measured the pH of the solution by changing its color depending on the concentration of H and OH ions

A

pH paper

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16
Q

pH paper is treated with an indicator known as

A

FLAVIN

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17
Q

flavin is an ____ commonly found in red cabbages

A

ANTHOCYANIN

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18
Q

flavin usually turns:

solution is acidic

A

RED

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19
Q

flavin usually turns:

solution is neutral

A

GREEN

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20
Q

flavin usually turns:

solution is basic

A

PURPLE

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21
Q
A
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22
Q
  • more accurate method than pH paper
  • contains a probe that passes the electrical signals to the meter itself which interprets the electrical signals and display the results on its screen
A

pH meter

23
Q

two electrodes of ph meter

A

sensor
reference

24
Q

contains a pH 7 buffer

A

sensor electrode

25
Q

usually contains saturated KCl solution

A

reference electrode

26
Q

made up of porous glass; have both a silver wire covered with silver chloride or calomel

A

PROBE

27
Q

pH meter probe has a silver wire that is covered with

A

silver chloride or calomel

28
Q
  • H ions are spontaneously generated in pure water by the dissociation (ionization) of a small percentage of water molecules
  • dissociation makes equal numbers of H and OH ions
  • while the OH ions can float around in solution as themselves, the H ions are transferred directly to a neighboring water molecule to form hydronium ions
A

AUTOIONIZATION OF WATER

29
Q

AUTOIONIZATION OF WATER

H+ spontaneously ____ to form H+ and OH- equally

A

DISSOCIATES

30
Q

the ____ of H+ causes it to bind to another H2O molecule, thus forming a hydronium ion

A

REACTIVITY

31
Q

AUTOIONIZATION OF WATER

The amount of dissociative H+ is ____ to the amount of H3O+ formed.

A

EQUAL

32
Q
  • Acids are species that increase [H+]
  • Bases are species that increase [OH-]
  • Limited in describing acidity and basicity to dissociation in aqueous solution
A

ARRHENIUS

33
Q

ARRHENIOUS

Many substances behave as an acid or base in ____ phase where no solvent is present

A

GASEOUS PHASE

34
Q

● Acids are proton donors
- Must have a H+ that can
dissociate

● Bases are proton acceptors
- Must have at least one pair of electrons to form a bond with a proton

A

BRONSTED-LOWRY

35
Q

BRONSTED

react almost completely with water

A

STRONGER ACIDS

inorganic acids

36
Q

react only slightly with water

A

WEAK ACIDS

acetic acid

37
Q

Acid strengths are given using what values

A

pKa

38
Q

acid dissociation constant

A

Ka

39
Q

gives the exact strength of acid in water

A

Ka
acid dissociation constant

40
Q

There is an ____ relationship between Ka and pKa

A

INVERSE

41
Q
  • Acids accept a pair of non-binding electrons
  • Bases donate a pair of non-binding electrons
  • Suggest that sharing electrons between acids and bases causes no change in the oxidation numbers of any atoms.
A

LEWIS

42
Q

Provided a way of simplifying the expression of [H+]

A

SORENSEN

43
Q

pH means

A

pruissance d’ hydrogen

44
Q

pruissance d’ hydrogen means

A

POWER OF HYDROGEN

45
Q

how to compute for pH & pOH

A

-log [H+]
-log {OH-]

46
Q

how to compute for [H+] [OH-]

A

10‾pH
10‾pOH

47
Q

formula for pKw

A

pKa + pKb = 14
pH + pOH = 14

48
Q
  • Resist change in pH
  • Most organisms, including humans, need to maintain pH within a fairly narrow range to survive
  • Consists of an acid-base pair, with the acid and base differing by the presence or absence of a proton (conjugate acid-base pair)
A

BUFFERS

49
Q

BUFFERS

human blood involves what acid

A

CARBONIC ACID
H₂CO₃

50
Q

BUFFER

conjugate base of the human blood

A

BICARBONATE ION
HCO₃‾

51
Q

Used to calculate the pH of a buffer system

A

HENDERSON-HASSELBALCH

52
Q

formula for buffer, weak acids

A

pH = pKa + log (salt/acid)

53
Q

formula for buffer, weak bases

A

pH = pKw - pKb + log (base/salt)

BIOCHEM LAB (11 decks)

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