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MODULE 5: Acids, Bases and pH

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Total cards: 12•Content version: v4•Public deck•Updated: 8/1/2026

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#1
Front (Question)

Bronsted-Lowry model of acids:

Back (Answer)

Acids are proton donators

#2
Front (Question)

Bronsted-Lowry model of bases:

Back (Answer)

Bases are proton acceptors

#3
Front (Question)

Conjugated acid-base pair:

Back (Answer)

Consists of two substances that differ only by the presence of a proton (H⁺) e.g. HCl releases a proton to form the conjugated base Cl-, Cl- accepts a proton to form a conjugated acid HCl

#4
Front (Question)

Conjugated acid-base pair of neutralisation:

Back (Answer)

HX + OH- –> H2O + X- OH- = conjugated base H2O = conjugated acid

#5
Front (Question)

Reaction of acids with metals:

Back (Answer)

acid + metal = salt + hydrogen gas

#6
Front (Question)

Neutralisation of acids with carbonates:

Back (Answer)

acid + carbonate = salt + water + carbon dioxide gas

#7
Front (Question)

Neutralisation of acids with metal oxides:

Back (Answer)

acid + metal oxide = salt + water

#8
Front (Question)

Neutralisation of acids with alkalis:

Back (Answer)

acid + alkali = salt + water

#9
Front (Question)

pH definition:

Back (Answer)

pH = -log10[H⁺]

#10
Front (Question)

Converting from pH to concentration of H⁺:

Back (Answer)

10^-pH

#11
Front (Question)

pH of strong acids:

Back (Answer)

Concentration of the acid is equal to the concentration of H⁺ as they fully dissociate

#12
Front (Question)

Acid dissociation constant (Ka):

Back (Answer)

Exactly the same as the rate equation, except used for weak acids to display the concentration of H⁺