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acids, bases, buffers

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

Card preview (24)

#1
Front (Question)

write an expression for how to calculate pH

Back (Answer)

pH = - log [H+]

#2
Front (Question)

explain how to calculate the pH of a strong acid

Back (Answer)

concentration of acid = [H+] because it is fully dissociated in water

#3
Front (Question)

what are the assumptions made in the calculation of a strong acid

Back (Answer)

the acid is full dissociated [acid] = [H+]

#4
Front (Question)

explain how to calculate [H+] from a given pH

Back (Answer)

[H+] = 10 to power of -pH

#5
Front (Question)

define bronsted lowry acid

Back (Answer)

proton donor

#6
Front (Question)

define bronsted lowry base

Back (Answer)

proton acceptor

#7
Front (Question)

explain the difference between a weak and strong acid

Back (Answer)

strong acids are fully dissociated in water, weak acids only partially dissociate in water

#8
Front (Question)

write the equation for the reaction of a strong acid with water

Back (Answer)

HA + H2O –> H3O+ + A-

#9
Front (Question)

write an equation for the reaction of a weak acid with water

Back (Answer)

HA + H20 ⇌ H3O+ + A-

#10
Front (Question)

explain how to calculate [H+] for H2SO4

Back (Answer)

2 x concentration of acid = [H+] because its diprotic

#11
Front (Question)

write an expression for the ionic product of water (Kw)

Back (Answer)

Kw = [H+] [OH-]

#12
Front (Question)

modify Kw to calculate the pH of pure water

Back (Answer)

Kw = [H+] squared

#13
Front (Question)

what assumption is made in the calculation of pH of pure water

Back (Answer)

that each water molecule dissociates to give H+ and OH-

#14
Front (Question)

explain how to calculate pH of a strong base

Back (Answer)

assume concentration of base is equal to [OH-] concentration , then use the Kw expression

#15
Front (Question)

explain how to calculate [OH-] of barium hydroxide

Back (Answer)

Ba(OH)2 therefore 2x the concentration of BaOH2 = [OH-]

#16
Front (Question)

explain why pure water is always neutral regardless of the pH

Back (Answer)

[H+] = [OH-] at any temperature for an acid [H+] > [OH-] for a base [H+] < [OH-]

#17
Front (Question)

calculate pKa

Back (Answer)

pKa = - log Ka

#18
Front (Question)

calculate Ka from pKa

Back (Answer)

Ka = 10 to power of -pKa

#19
Front (Question)

write an expression for Ka

Back (Answer)

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

#20
Front (Question)

define a buffer solution

Back (Answer)

a solution that resists the change in pH when a small amount of acid or alkali are added

#21
Front (Question)

write a modified expression for Ka when doing buffer calculation

Back (Answer)

Ka = [H+] x (salt/acid)

#22
Front (Question)

how do you make a buffer

Back (Answer)

mixture of a weak acid and it’s sodium salt

#23
Front (Question)

what happens to the reaction of HA reversible reaction arrow when NaOH is added when a buffer is present

Back (Answer)

H+ + OH- —> H2O concentration of H+ ions decreases therefore equilibrium shifts to right no change in pH

#24
Front (Question)

write an equation for the disassociation of a weak acid HA

Back (Answer)

HA ⇌ H+ + A-