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Organic Chemistry Lab > Module 2: ACIDITY AND BASICITY OF ORGANIC COMPOUNDS > Flashcards

Module 2: ACIDITY AND BASICITY OF ORGANIC COMPOUNDS Flashcards

1
Q
  • acids and bases are defined through three main concepts:
A

✓ Arrhenius Theory
✓ Brønsted-Lowry Theory
✓ Lewis electron pair Theory

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2
Q

BRønsted-Lowry Theory

  • a “base” is any species that can _________________
  • a Brønsted-Lowry base must have at least one lone pair of electron to be able to form bond with a proton
A

accept a proton

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2
Q

gives the exact strength of a given acid in water

A

Ka (acidity constant)

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3
Q

ArrHenius Theory

  • “acid” is any species that can increase the concentration of ______________ in an aqueous solution
A

hydrogen ions (protons)

HCl → H+ + Cl–

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3
Q

ArrHenius Theory

  • “base” is any species that can increase the concentration of _____________ in an aqueous solution
A

hydroxide ions, OH–,

NaOH → Na+ + OH–

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4
Q

BRønsted-Lowry Theory

  • an “acid” is any species that can _________________________
  • a Brønsted-Lowry acid must have a hydrogen that can dissociate as H+
A

donate a proton (H+)

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4
Q

___________ react almost completely with water

A

stronger acids (eg. inorganic acids)

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5
Q

Lewis “electron” pair Theory

  • an “acid” is a species that can _______________
A

accept a pair of non-bonding electrons

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5
Q

in a Brønsted-Lowry acid-base reaction

a _______________ is the species formed after an acid donates its proton

A

conjugate base

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5
Q

HCl (aq) + H2O (l) → H3O+(aq) + Cl–(aq)

__________ acts as the Brønsted-Lowry acid; __________ is the conjugate base of HCl

A
  1. HCl
  2. Cl
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5
Q

react only slightly with water

A

weak acids (eg. acetic acid)

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5
Q

HCl (aq) + H2O (l) → H3O+(aq) + Cl–(aq)

__________ is the Brønsted-Lowry base; ________
is the conjugate acid of the water

A
  1. H2O
  2. H3O+
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5
Q

in a Brønsted-Lowry acid-base reaction

____________ is a species formed after the base accepts a proton

A

conjugate acid

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5
Q

acid strengths are normally given using

A

pKa values (pKa = –log Ka)

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6
Q
  • note that the negative logarithm in the definition of pKa indicates an _____________ between Ka and pKa
A

inverse relationship

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6
Q

Lewis electron pair Theory

  • suggest that acids react with bases, ___________, with no change in the oxidation numbers of any atoms
A

sharing a pair of electrons

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6
Q

Lewis electron pair Theory

  • a “base” is a species that can ________________
A

donate a pair of non-bonding electrons

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6
Q

pOH

A

power of hydroxide

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7
Q
  • the Lewis structure of “water” shows that it has a _________________________, therefore acting as the Lewis base
A

non-bonding pairs of valence electrons

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8
Q
  • the reaction between a Lewis acid and a Lewis base gives rise to an _______________
A

acid-base complex or complex ion

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8
Q
  • the “aluminum ion” (Al3+) suggests that it has free orbitals that can ________________________ donated by the water molecules, thereby acting as the Lewis acid
A

accept pairs of non-bonding electrons

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9
Q

pH means

A

power of hydrogen

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10
Q
  • the acidity and basicity of a substance can be measured in terms of the molar ___________________________ ions, respectively
A

concentration of the hydrogen (H+) or hydroxide (OH–)

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10
Q
  • pOH is defined as the _________________ ion concentration of a substance
A

negative logarithm of the OH–

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10
Q
  • pH is defined as the _________________ ion concentration of a substance
A

negative logarithm of the H+

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11
Q

pH of battery acid

A

0 pH

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12
Q

pH of stomach acid

A

1 pH

13
Q

pH of vinegar

A

2 pH

14
Q

pH of tomato

A

4 pH

14
Q

pH of baking soda

A

9 pH

15
Q

pH of orange juice

A

3 pH

15
Q

pH of sea water

A

8 pH

15
Q

pH of black coffee

A

5 pH

16
Q

pH of urine

A

6 pH

16
Q

pH of indigestion tablet

A

10 pH

16
Q

pH of water

A

7 pH

17
Q

8 - 14 pH

A

Base (alkali)

17
Q

pH of ammonia solution

A

11 pH

17
Q

neutral pH

A

7

17
Q

pH of bleach

A

13 pH

18
Q

0 - 6 pH

A

Acid

18
Q

pH of soapy water

A

12 pH

19
Q

pH of drain cleaner

A

14 pH

20
Q
  • the pH of a solution may be measured using _____________
A

pH paper

20
Q
  • pH paper measures the pH of the solution by __________________ depending on the concentration of H+ and OH–ions
A

changing its color

21
Q
  • this paper is treated with an indicator, which is ______________, an “anthocyanin” commonly found in “red cabbages”
A

flavin

22
Q
  • this paper is treated with an indicator, which is flavin, an ___________ commonly found in red __________________
A
  1. anthocyanin
  2. red cabbages
23
Q
  • flavin usually turns:
  • ___________ if the solution is acidic
  • ___________ if the solution is neutral
  • ___________ if the solution is basic
A
  1. red
  2. greenish
  3. purple
24
Q
  • ________________ is a more accurate method than pH paper
A

pH meter

25
Q
  • contains a _____________that passes the electrical signals to the meter itself which interprets the electrical signals and display the results on its screen
A

probe

26
Q
  • the glass pH probe contains two electrodes:

____________ that contains a pH 7 buffer
solution

A

sensor electrode

27
Q
  • the glass pH probe contains two electrodes:

_______________ that usually contains saturated potassium chloride solution

A

reference electrode

28
Q
  • these electrodes made up of porous glass have both a silver wire covered with ________________
A

silver chloride or calomel

29
Q
  • when the probe is immersed in a solution, the ____________ accumulate around the bulb of the electrode, generating an electrical flow
    captured by the silver wire
A

hydrogen ions

30
Q
  • the _____________ is measured by the meter and then converts it to pH value
A

voltage of this electrical flow

31
Q

CLASSIFICATION OF pH
= 0.1 M acetic acid

A

acidic (weak)

32
Q

CLASSIFICATION OF pH
= 0.1 M acetamide

A

basic (weak)

33
Q

CLASSIFICATION OF pH
= 0.1 M phenol

A

acidic (weak)

34
Q

CLASSIFICATION OF pH
= aniline

A

basic (weak)

34
Q

CLASSIFICATION OF pH
= 0.1 M glycine

A

neutral (theoretically)

35
Q

CLASSIFICATION OF pH
= 1% glucose

A

neutral (theoretically)

36
Q

CLASSIFICATION OF pH
= acetone

A

acidic to neutral

37
Q

CLASSIFICATION OF pH
= isopropyl alcohol

A

acidic (weak)

38
Q

pH scale allows us to easily classify substances based on their acidity and basicity at ____________

A

25°C

39
Q

indicator of pH paper

A

flavin

Organic Chemistry Lab (6 decks)

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