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Chemistry > Acids & Bases > Flashcards

Acids & Bases Flashcards

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1
Q

Definition of acid

A

Proton donor

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2
Q

Definition of base

A

Proton acceptor

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3
Q

Definition of strong acid

A

An acid which fully dissociates

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4
Q

Definition of weak acid

A

An acid which partially dissociates

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5
Q

Definition of pH

A

pH = -log10 [H+]

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6
Q

Definition of [H+]

A

[H+] = 10-pH

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7
Q

Ionic product of water (Kw)

A

Kw = [H+][OH-]

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8
Q

Calculating pH of strong acid

A

pH = -log10 [H+]

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9
Q

Calculating pH of a strong base

A

Rearrange Kw = [H+][OH-] to get [OH-]
then use pH = -log10 [H+]

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10
Q

Calculating pH of a weak acid

A

Ka = [H+]2 ÷ [HA]
and rearrange to get [H+]

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11
Q

Calculating pH of a buffer

A

Ka = [H+][A-] ÷ [HA]
and rearrange to get [H+]

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12
Q

Acid + Metal →

A

Acid + Metal →Salt + Hydrogen

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13
Q

Acid + Metal Oxide →

A

Acid + Metal Oxide →Salt + Water

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14
Q

Acid + Metal Hydroxide →

A

Acid + Metal Hydroxide → Salt + Water

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15
Q

Acid + Metal Carbonate →

A

Acid + Metal Carbonate →Salt + CO2 + Water

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16
Q

Examples of strong acids:

A

HCl
H2SO4
HNO3
H3PO4

17
Q

Group 1 is called the ‘Alkali Metals’ and Group 2 is called the ‘Alkaline Earth Metals’. As such the oxides of Na and Mg are both alkaline and react with water to form basic solutions

A

Eg:

Na2O(s) + H2O(l) → 2Na+(aq) + 2-OH(aq

MgO(s) + H2O(l) → Mg(OH)2(aq)

18
Q

Period 3 Oxides:
Magnesium hydroxide

A

Magnesium hydroxide is sparingly soluble and so is weakly alkaline

19
Q

Acids:

A

Any substance which dissociates to release H+ ions is classed as an acid

20
Q

Base:

A

Any substance which will accept and bond to an H+ ion is classed as a base

21
Q

Definition of amphoteric

A

When water can act as an acid or a base

22
Q

Key points of pH scale:

A

1) The smaller the pH, the greater the concentration of H+ ions
2) A difference of 1 on pH scale means a 10x difference in [H+]
3) It is possible to have a pH below 0 for very strong acids and a pH above 14 for a very strong base

23
Q

pH for diprotic acids and triprotic acids
eg: H2SO4 & H3PO4

A

pH = -log10 [H+ × 2]

pH = -log10 [H+ × 3]

24
Q

Method for weak acid pH calculations:

A

1) write out dissociation of weak acid
2) construct a Ka expression for the acid
3) simplify Ka expression using [H+]2
4) rearrange expression to get [H+] on its own
5) substitute value of [H+] I to pH equation

25
Q

pKa

A

pKa = -log10Ka

26
Q

Ka

A

Ka = 10-pKa

27
Q

Kw is called the ionic product of water and at 298K has a value of 1x10-14mol2dm-6

The value of Kw will alter with temperature

A
28
Q

Why is pure water always neutral?

A

[H+] = [OH-] at all times

Chemistry (9 decks)

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