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Chemistry (J1) > 15 Acid-Base Equilibria > Flashcards

15 Acid-Base Equilibria Flashcards

1
Q

Arrhenius Theory

A

An acid is a compound that dissolves in water to yield hydrogen ions
A base is a compound that dissolves in water to yield hydroxide ions

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2
Q

Bronsted-Lowery Theory

A
  • An acid is a substance that donates a proton to another substance
  • A base is a substance that accepts a proton from another substance
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3
Q

Lewis Theory

A
  • An acid is a substance that can accept a pair of electrons from a base to form a dative covalent bond
  • A base is a substance that can donate a pair of electrons to an acid to form a dative bond
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4
Q

Strong acid/base

A

Ionizes completely in aqueous solutions

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5
Q

Weak acid/base

A

Ionizes partially in aqueous solutions

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6
Q

Degree of ionisation, α

A

amount of molecules which ionised at equilibrium/
amount of molecules present initially

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7
Q

pH

A

pH = -lg [H+]
[H+] = 10^-pH

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8
Q

pOH

A

pOH = -lg [OH-]
[OH-] = 10^-pOH

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9
Q

Ionic product of water, Kw

A

Kw = [H+][OH-]
Kw at 25°C = 1.00 *10^-4 mol^2 dm^-6

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10
Q

Relationship between p Kw, pH, pOH

A

p Kw = pH + pOH (=14 at 25°C)

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11
Q

Acid dissociation constant, Ka

A

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

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12
Q

p Ka

A

-lg Ka

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13
Q

Base dissociation constant, Kb

A

Kb = [BH+][OH-]/[B]

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14
Q

p Kb

A

-lg Kb

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15
Q

Conjugate acid-base pair

A

An acid and a base differing by the presence or absence of a proton

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16
Q

Relationship between Ka, Kb and Kw

A

Ka*Kb = Kw = 1.00 *10^-4 mol^2 dm^-6 (at 25°C)
p Ka + p Kb = p Kw (= 14 at 25°C)

17
Q

pH of salt of strong acid + strong base

A

7 (neutral)

18
Q

pH of salt of weak acid + strong base

A

> 7 (basic)

19
Q

pH of salt of strong acid + weak base

A

<7 (acidic)

20
Q

pH of salt of weak acid + weak base

A

depends on Ka and Kb of resulting conjugate acid/base

21
Q

Buffer solution

A

A buffer solution is one that can resist a change in pH when a small amount of acid/base is added to it

22
Q

Acidic buffer solution

A

A solution with a weak acid and its conjugate base

23
Q

Basic buffer solution

A

A solution with a weak base and its conjugate acid

24
Q

Henderson-Hasselbalch Equation

A

pH= p Ka + lg ([A-]/[HA])
pOH= p Kb + lg ([BH+]/[B])

25
Q

Maximum buffering capacity

A

[HA] = [A-], pH = p Ka
[B] = [BH+], pOH = p Kb

26
Q

Buffer solution in blood

A

H2CO3/(HCO3)- buffer

27
Q

Equivalence point

A

The point during a titration at which stoichiometric amounts of reactants have reacted

28
Q

End point

A

The point during a titration when the indicator changes colour

29
Q

Acid-base indicator

A

A substance which shows different colours in solutions of different pH

Chemistry (J1) (15 decks)

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