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Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

What is a Bronsted Lowry acid

A

A proton donnor

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2
Q

What is a Bronsted Lowry base

A

A proton acceptor

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3
Q

What does acid base equilibria involve?

A

The transfer of protons

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4
Q

Why do we use the log scale for hydrogen ion concentration

A

It covers a very wide range

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5
Q

What is the pH formula

A

pH = -log10[H+]

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6
Q

What is the kw formula used for?

A

Water and Strong bases

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7
Q

What is the Kw formula

A

Kw = [H+][OH-]

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8
Q

How does the value of kw vary

A

With temperature

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9
Q

How is Kw special for pure water

A

Kw = [H+]^2

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10
Q

How can water act?

A

As both an acid and a base.
It can lose or gain an H+

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11
Q

Why does the pH of water change with temperature

A

The forward reaction will be favoured, and more hydrogen ions and hydroxide ions will be formed. The effect of that is to increase the value of Kw as temperature increases.

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12
Q

How do weak acids and bases dissociate

A

Only slightly

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13
Q

What is the dissociation constant of a weak acid

A

Ka

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14
Q

What is pKa equal to

A

-log10Ka

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15
Q

What do we assume for weak acids

A

No dissociation

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16
Q

What does assuming no dissociation mean for a weak acid

A

[H+] = [A-]
This means making H+ squared instead of A- and H= separately

17
Q

What is the formula for Ka

A

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

18
Q

How do you work out pH of a strong acid

A

Assume complete dissociation e.g. 0.16mol dm-3 of HCl
[H+] = 0.16

19
Q

What does a graph of a strong acid and strong base look like

A

Low starting pH and high end pH.
Long equivalence point

20
Q

What does a graph of a strong acid and weak base look like

A

Low starting pH and just above neutral end pH.
Short equivalence point

21
Q

What does a graph of a weak acid and strong base look like

A

Starting pH not far below neutral and high end pH.
Short equivalence point

22
Q

What does a graph of a weak acid and weak base look like

A

Starting pH not far below neutral and just above neutral end pH.
Very short equivalence point

23
Q

What does a buffer pH do?

A

Maintains a constant pH

24
Q

What do acidic buffers contain?

A

A weak acid and the salt of that weak acid

25
Q

What do basic buffers contain?

A

A weak base and the salt of that weak base

26
Q

What is the equivalence point?

A

Just enough acid has been added to neutralise the base or visa versa

27
Q

What goes in an ice table

A

Moles

28
Q

A buffer solution has a constant pH even when diluted. Use a mathematical expression to explain this.

A

Chemistry (36 decks)

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