Back to marketplace

Unit 1: Section 9 - Acids, Bases and pH

No description yet. This curated deck is ready for daily study.

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

Card preview (24)

#1
Front (Question)

Define a Bronsted-Lowry acid

Back (Answer)

Proton donor

#2
Front (Question)

Define a Bronsted Lowry base

Back (Answer)

Proton acceptor

#3
Front (Question)

What ion causes a solution to be acidic? ( answers) Name and formula

Back (Answer)

H+, or more accurately H3O+ (oxonium ion), as protons react with H2O to form it

#4
Front (Question)

What ion causes a solution to be alkaline?

Back (Answer)

-OH (hydroxide ion)

#5
Front (Question)

Write an equation for the ionisation of water (2)

Back (Answer)

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

#6
Front (Question)

Derive Kw using the equation for the ionisation of water

Back (Answer)

Keq = [H+] [OH-] / [H2O] [H2O]Keq = [H+] [OH-] [H2O] is so large compared to [H+] and [Oh-] that [H2O]Keq can be considered to be constant. [H2O]Keq = Kw ∴ 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)

Temperature only - if temperature is increased, the equilibrium moves to the right Kw increases and the pH of pure water decreases

#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)

If 2 solutions have a pH difference of 1, what is the difference in [H+]?

Back (Answer)

A factor of 10

#13
Front (Question)

How do you find [H+] from pH?

Back (Answer)

[H+] = 10^-pH

#14
Front (Question)

How do you find [OH-] from pH?

Back (Answer)

Find [H+], use Kw to calculate [OH-]

#15
Front (Question)

What is the difference when finding [H+] from the concentrations of diprotic and tripotic acids?

Back (Answer)

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 in water ( HX -> H+ + X-)

#18
Front (Question)

Define the term strong base

Back (Answer)

One which fully dissociates in water (XOH -> X+ + OH-)

#19
Front (Question)

What is the difference between concentrated and strong?

Back (Answer)

Concentrated means many mol per dm^3, strong refers to amount of dissociation

#20
Front (Question)

What is a weak acid and a weak base?

Back (Answer)

• They only partially dissociate into their ions

#21
Front (Question)

Give some examples of strong acids

Back (Answer)

HCl, H2SO4 and H3PO4

#22
Front (Question)

Give some examples of strong bases

Back (Answer)

NaOH, CaCO3 and Na2CO3

#23
Front (Question)

Give some examples of weak acids

Back (Answer)

CH3COOH (ethanoic), any organic acid

#24
Front (Question)

Give some examples of weak bases

Back (Answer)

NH3