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1.12 Acids and Bases

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

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#1
Front (Question)

Define a Bronstead-Lowry acid

Back (Answer)

A proton donor

#2
Front (Question)

Define a Bronstead-Lowry base

Back (Answer)

Proton acceptor

#3
Front (Question)

What ion causes a solution to be acidic ?

Back (Answer)

• H+ (hydrogen ion) • H3O+ (Oxonium ion).

#4
Front (Question)

What ion causes a solution to be alkaline ?

Back (Answer)

Hydroxide ion (OH-)

#5
Front (Question)

Write an equation for the ionisation of water

Back (Answer)

• 2H2O (l) ⇌ H3O+ (aq) + OH- (aq) • H2O (l) ⇌ H+ (aq) + OH- (aq).

#6
Front (Question)

Derive Kw using the formula for the ionisation of water

Back (Answer)

• Kc = [H+][OH-] / [H2O] • Kc [H2O] = [H+][OH-] • [H2O] is so large that it can be assumed that it is constant • Therefore Kw = [H+][OH-].

#7
Front (Question)

What is the value of Kw at 298K

Back (Answer)

1.0 x 10 ⁻¹⁴

#8
Front (Question)

What physical factors affect the value of Kw? How do they affect it?

Back (Answer)

• Only temperature effects the value of Kw • If temperature increases, the equilibrium moves to the right • Kw increases therefore and the pH of pure water increases.

#9
Front (Question)

Why is pure water still neutral, even if pH does not equal 7 ?

Back (Answer)

[H+] = [OH-]

#10
Front (Question)

Give an expression for pH in terms of H+

Back (Answer)

pH = -log([H+])

#11
Front (Question)

What is the relationship between pH and concentration of H+?

Back (Answer)

Lower pH = higher concentration of H+.

#12
Front (Question)

By what scale does the concentration of H+ increase if you jump from pH 2 to 1 ?

Back (Answer)

x10.

#13
Front (Question)

How do you find the [H+] from pH ?

Back (Answer)

[H+] = 10 ⁻ᵖᴴ

#14
Front (Question)

How do you find [OH-] from pH ? (298K)

Back (Answer)

• Find [H+] • Use Kw / [H+] = [OH-].

#15
Front (Question)

What is different when finding the concentration of H+ in diprotic and triprotic acids ?

Back (Answer)

You need to multiply the concentration of the acid by the number of protons to find [H+].

#16
Front (Question)

How do you calculate the pH of a strong alkaline solution ?

Back (Answer)

• Use Kw to calculate [H+] from [OH-] • Use pH = -log([H+])

#17
Front (Question)

Define the term strong acid

Back (Answer)

One which fully dissociates into water : XH -> X- + H+.

#18
Front (Question)

Define the term strong base

Back (Answer)

One which fully dissociates into water: XOH -> X+ + OH-

#19
Front (Question)

What is the difference between a concentrated acid and strong acid ?

Back (Answer)

• Concentrated means many moles per dm3 • Strong refers to amount of dissociation.

#20
Front (Question)

What are weak acids and bases ?

Back (Answer)

Acids / bases which only partially dissociate into their ions in a solution.

#21
Front (Question)

Give some examples of strong acids

Back (Answer)

HCl, H2SO4, HNO3, H3PO4

#22
Front (Question)

Give some examples of strong bases

Back (Answer)

NaOH, CaCO3, Na2CO3

#23
Front (Question)

Give an example of a weak acid

Back (Answer)

CH3COOH, any organic acid.

#24
Front (Question)

Give an example of a weak base

Back (Answer)

NH3