chapter 20 Flashcards

1
Q

What is a Brønsted Lowry acid?

A

a species that can donate a proton

hydrogen chloride (HCl) is a Brønsted acid as it can lose a proton to form a hydrogen (H+) and chloride (Cl-) ion

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2
Q

What is a Brønsted Lowry base?

A

a species that can accept a proton

A hydroxide (OH-) ion is a Brønsted base as it can accept a proton to form water

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3
Q

What is a conjugate acid-base pair?

A

A conjugate acid-base pair is two species that are different from each other by an H+ ion.

CH3COOH (aq) + H2O (l) ⇌ CH3COO- (aq) + H3O+ (aq)

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4
Q

What does it mean for an acid to be classified as mono basic/dibasic or tribasic?

A

It means the number of bases that they can donate protons to in a reaction (this depends on how many H+ per molecule that they can give up in a reaction)

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5
Q

Example of mono basic acid + what this means

A

HCL, It contains one ionisable hydrogen atom in each molecule.

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6
Q

Example of dibasic acid + what this means

A

H2SO4, It contains two ionisable hydrogen atoms per molecule. Ionisation occurs in two steps.

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7
Q

Example of tribasic acid + what this means

A

H3PO4, It contains 3 ionisable hydrogen atoms per molecule. Ionisation occurs in 3 steps.

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8
Q

Acid + metal =

A

acid + metal → salt + hydrogen

2HCl (aq) + Zn (s) → ZnCl2 (aq) + H2 (g)

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9
Q

acid + metal oxide =

A

acid + metal oxide → salt + water

2HCl (aq) + CaO (s) → CaCl2 (aq) + H2O (l)

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10
Q

acid + metal carbonate =

A

acid + metal carbonate → salt + water + carbon dioxide

2HNO3 (aq) + CuCO3 (s) → Cu(NO3)2 (aq) + H2O (l) + CO2 (g)
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11
Q

acid + alkali =

A

acid + alkali → salt + water

HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)

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12
Q

What is a weak acid?

A

A weak acid is an acid that partially (or incompletely) dissociates in aqueous solutions.

eg. ethanoic acid/ carbonic acid

(equilibrium is more to the left- there are lots more weak acid molecules than H+ and A- Ions.)

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13
Q

What is the equilibrium constant for a weak acid?

A

Ka

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14
Q

What is the equilibrium constant expression for Ka?

A

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

this can be simplified to [H]^2 / [HA]

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15
Q

What are the units of Ka?

A

mol dm-3

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16
Q

A high Ka value means…?

A

The higher the value of Ka the more dissociated the acid and the stronger it is

17
Q

A low Ka value means….?

A

The lower the value of Ka the weaker the acid

18
Q

Why do we use pka instead of Ka?

A

Its difficult to compare numbers with negative indices, so we use pka as it is whole numbers.

19
Q

How do you go from Ka to pKa?

A

pKa = -log(Ka)

20
Q

How do you go from pKa to Ka?

A

Ka = 10^-(pKa)

21
Q

A high pKa value means…?

A

The acid is weak.

22
Q

A low pKa value means…?

A

The acid is strong and more dissociated.

23
Q

How do you work out pH?

A

pH= -log[H+]

H+ = conc of hydrogen atoms in moldm-3

24
Q

How do you calculate [H+] with the pH?

A

[H+] = 10^-pH

25
Q

How much does each pH value differ by?

A

The pH scale is a logarithmic scale with base 10
This means that each value is 10 times the value below it.

pH 1 = 10^-1
PH 2 = 10^-2

26
Q

What is the ionic product of water?

A

Kw

27
Q

What’s the value of Kw?

A

1 x 10^-14 mol^2dm^-6 @ 298k

28
Q

What’s the equation for Kw?

A

Kw = [H+][OH-] / [H20]

Kw x [H20] = [H+][OH-]

29
Q

What approximations are made with Ka?

A

HA dissociates to create concentrations of H+ and A-
this is what allows us to write [H+]^2. We also ignore the very small conc of H+ from water dissociating.

As the dissociation of weak acids is small we assume that the concentration of the weak acid is the same at the start and the end.

30
Q

How do you work out pH with Ka?

A

square root of Ka x [HA] = H+
so you then do -log[H+]

31
Q

How do you calculate the pH of a strong acid?

A

Strong acids completely ionise within solution.

So [H+] = [HA]

32
Q

How do you calculate the pH of a strong base?

A

Strong bases completely ionise within solution.

So H+ = Kw (1x10^-14) / [OH-]

You then use the H+ to work out pH.

Kw = [OH-] x [H+]