PHYSICAL CHEM - ACIDS AND BASES

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

Card preview (24)

Front (Question)

What is a Bronsted-Lowry acid?

Back (Answer)

a proton donor

Front (Question)

What is a Bronsted-Lowry base?

Back (Answer)

a proton acceptor

Front (Question)

What is a strong acid?

Back (Answer)

an acid that completely dissociates into H^+ ions/ionises in water/aqueous solution

Front (Question)

What is a weak acid?

Back (Answer)

an acid that only partially dissociates into H^+ ions/ionises in water/aqueous solution

Front (Question)

What is a strong base?

Back (Answer)

a base that completely dissociates into OH^- ions/ionises in water/aqueous solution

Front (Question)

What is a weak base?

Back (Answer)

a base that only partially dissociates into OH^- ions/ionises in water/aqueous solution

Front (Question)

Where does equilibrium lie when strong acids/bases dissociate into their ions?

Back (Answer)

extremely far to the right

Front (Question)

Where does equilibrium lie when weak acids/bases dissociate into their ions?

Back (Answer)

to the left

Front (Question)

What is the equation for the dissociation of water?

Back (Answer)

H2O + H2O ⇌ H3O^+ + OH^-

#10

Front (Question)

Where does equilibrium lie in the dissociation of water and why?

Back (Answer)

• far to the left • only dissociates a tiny amount

#11

Front (Question)

What is the equation for pH?

Back (Answer)

pH = - log [H^+]

#12

Front (Question)

What is the equation for the conc. of H^+ ions?

Back (Answer)

[H^+] = 10^-pH

#13

Front (Question)

What is the equation for Kw?

Back (Answer)

Kw = [H^+][OH^-]

#14

Front (Question)

What is the value of Kw at 298K/25°C?

Back (Answer)

1 x 10^-14

#15

Front (Question)

How does the pH of water change as temp increases and why?

Back (Answer)

• as temp increases water becomes more acidic • the forward reaction in the equilibrium of water is endothermic and is therefore favoured when temperature of the water increases • therefore more H^+ ions are produced

#16

Front (Question)

What is Ka?

Back (Answer)

• weak acids and bases only slightly dissociate in solution to form an equilibrium mixture • therefore the reaction has an equilibrium dissociation constant (Ka)

#17

Front (Question)

What is the equation for Ka?

Back (Answer)

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

#18

Front (Question)

What is the equation for pKa?

Back (Answer)

pKa = - log (Ka)

#19

Front (Question)

How can you find the pH of a weak acid/base when HA is in excess?

Back (Answer)

use [HA] and [A^-] along with Ka to find [H^+], then find pH

#20

Front (Question)

How can you find the pH of a weak acid/base when A^- is in excess?

Back (Answer)

use Kw to find [H^+], then find pH

#21

Front (Question)

How can you find the pH of a weak acid/base when HA = A^-?

Back (Answer)

pKa = pH so find pKa

#22

Front (Question)

What is a titration curve?

Back (Answer)

• a graph that shows how pH of a solution changes during an acid-base reaction

#23

Front (Question)

What are the 4 types of titration curve?

Back (Answer)

• strong acid + strong base • strong acid + weak base • weak acid + strong base • weak acid + weak base

#24

Front (Question)

What is a buffer solution?

Back (Answer)

• a solution that minimises changes in pH when small amounts of an acid/base are added • work by neutralising added H^+/OH^- ions