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5.1.3 acids bases and buffers

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Total cards: 19•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (19)

#1
Front (Question)

Bronsted lowry acid

Back (Answer)

a substance that can donate a proton

#2
Front (Question)

Bronsted-Lowry base

Back (Answer)

Substance that can accept a proton

#3
Front (Question)

Bigger ka

Back (Answer)

stronger acid

#4
Front (Question)

Acid + metal

Back (Answer)

Salt + hydrogen

#5
Front (Question)

Acid + alkali

Back (Answer)

Salt + water

#6
Front (Question)

Acid + carbonate

Back (Answer)

Salt + water + co2

#7
Front (Question)

Ph equation

Back (Answer)

PH = -log [H+]

#8
Front (Question)

Strong acids

Back (Answer)

Completely dissociate in aqueous solutions E.g. HCl, HNO3

#9
Front (Question)

[H+] equation from pH

Back (Answer)

[H+]= 1x10^-pH

#10
Front (Question)

Ionic product for water

Back (Answer)

Kw = [H+] [OH-] Used for finding pH of pure water or pH of strong base when given [OH-] 1x10^-14 mol2 dm-6 At 25C

#11
Front (Question)

PH of strong base

Back (Answer)

[H+] = Kw / [OH-] PH = - log [H+]

#12
Front (Question)

Weak acids

Back (Answer)

Partially dissociate in aqueous solutions Ka = [H+][A-] / [HA]

#13
Front (Question)

pKa

Back (Answer)

pKa = -log [Ka] Ka = 10^-pKa

#14
Front (Question)

PH of diluted strong acid

Back (Answer)

[H+] = [H+]old x (old volume/new volume) Ph= -log [H+]

#15
Front (Question)

PH of diluted base

Back (Answer)

[OH-] = [OH-]old x (old volume/new volume) [H+] = kw / OH- PH = -log [H+]

#16
Front (Question)

Acidic buffer

Back (Answer)

Weak acid and salt of that weak acid

#17
Front (Question)

Basic buffer

Back (Answer)

Weak base and salt of that weak base

#18
Front (Question)

Adding small amounts of acid to buffer

Back (Answer)

Equilibrium shifts to left removing H+ ions added Large concentration of salt ion in buffer so ratio stays constant and pH stays constant

#19
Front (Question)

Adding small amount of alkali to buffer

Back (Answer)

OH- ions react with H+ to form water Equilibrium shifts to right to produce H+ ions Concentrations of H+ ions and pH remains constant