(I) Topic 21 - Acids and Bases

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

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Front (Question)

How does temperature increase effect the pH of water?

Back (Answer)

As the temperature increases, the equilibrium moves right to oppose the increase in temperature. [H+] and [OH-] increase. This causes Kw to increase, and pH to decrease.

Front (Question)

How does temperature increase effect the neutrality of water?

Back (Answer)

The water is still neutral as [H+] still equals [OH-]

Front (Question)

What is the difference between a strong and weak acid?

Back (Answer)

Strong acids fully dissociate whilst weak acids do not (only a fraction of the molecules break apart to form ions)

Front (Question)

Common strong monoprotic acids

Back (Answer)

Hydrochloric and Nitric Acid

Front (Question)

Common Weak Monoprotic Acids

Back (Answer)

Carboxylic Acids

Front (Question)

Common Strong Diprotic Acids

Back (Answer)

Sulfuric Acid

Front (Question)

Common strong monoprotic bases

Back (Answer)

Sodium and Potassium Hydroxide - NaOH and KOH

Front (Question)

Common strong diprotic bases

Back (Answer)

Barium Hydroxide - Ba(OH)2

Front (Question)

Common weak monoprotic bases

Back (Answer)

Ammonia

#10

Front (Question)

What are our assumptions when using Ka?

Back (Answer)

• [H+] = [A-] • [HA] at equilibrium is the same as at the start

#11

Front (Question)

What are the units of Ka?

Back (Answer)

moldm^(-3)

#12

Front (Question)

Are larger values of Ka weaker or stronger acids?

Back (Answer)

Stronger

#13

Front (Question)

Are larger values of pKa weaker or stronger acids

Back (Answer)

weaker

#14

Front (Question)

When do we use Ka?

Back (Answer)

For weak acids in aqueous solution with nothing else added

#15

Front (Question)

Titration Calculation Ionic Equation: H(+) + OH(-) ->

Back (Answer)

H2O

#16

Front (Question)

Titration Calculation Ionic Equation: 2H(+) + CO3(2-) ->

Back (Answer)

CO2 + H2O

#17

Front (Question)

Titration Calculation Ionic Equation: H(+) + HCO3(-) ->

Back (Answer)

H2O + CO2

#18

Front (Question)

Titration Calculation Ionic Equation: H(+) + NH3 ->

Back (Answer)

NH4(+)

#19

Front (Question)

What are indicators?

Back (Answer)

Indicators are weak acids where HA and A- are different colours. At lower pH, HA is the main species, at higher pH A- is, causing a colour change

#20

Front (Question)

Describe: Properties of methyl orange Include colour of HA, A- and pH range of colour change

Back (Answer)

HA= red A- = yellow pH range = 3.2 - 4.4

#21

Front (Question)

Describe: Properties of Phenolphhalein Include colour of HA, A- and pH range of colour change

Back (Answer)

HA = colourless A- = pink pH range = 8.2 - 10.0

#22

Front (Question)

What are, and are not appropriate indicators to use in a pH titration?

Back (Answer)

Appropriate: Methyl Orange, Phenolphthalein Inappropriate: Universal Indicator

#23

Front (Question)

What do pH curves show?

Back (Answer)

How the pH changes as an alkali is added to an acid or vice versa Rough Idea Okay

#24

Front (Question)

What is the equivilance point?

Back (Answer)

The point when the moles of alkali added equals the moles of acid present (The pH at the equivilance point is not always 7) • the pH at equivilance is about halfway up the characteristic steep section of the pH curve