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Acids, bases and buffers

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

Card preview (24)

#1
Front (Question)

Lewis acid

Back (Answer)

electron pair acceptor

#2
Front (Question)

Lewis base

Back (Answer)

electron pair donor

#3
Front (Question)

Bronsted Lowry base

Back (Answer)

proton acceptor

#4
Front (Question)

Bronsted-Lowry acid

Back (Answer)

proton donor

#5
Front (Question)

Dibasic acid

Back (Answer)

can form 2 conjugate bases

#6
Front (Question)

Conjugate acid base

Back (Answer)

HA + B -> HB+ + A- acid + base Conjugate acid + conjugate base

#7
Front (Question)

tribasic acid

Back (Answer)

can form 3 conjugate bases

#8
Front (Question)

Strong acid

Back (Answer)

completely dissociate in aqueous solutions to produce H+ ions large Ka smaller pKa

#9
Front (Question)

Weak acid

Back (Answer)

partially dissociate in aqueous solutions to produce H+ ions small Ka larger pKa

#10
Front (Question)

Acid dissociation constant

Back (Answer)

ka = [H+][A-] / [HA] = [H+]^2/[HA]

#11
Front (Question)

pH

Back (Answer)

-log10[H+] measure of hydrogen ion concentration in solution

#12
Front (Question)

[H+] from pH

Back (Answer)

10^-pH

#13
Front (Question)

[H+] from acid dissociation constant

Back (Answer)

√(ka x [HA])

#14
Front (Question)

pKa

Back (Answer)

-log10Ka

#15
Front (Question)

Ionic product of water formula

Back (Answer)

Kw = [OH-][H+] = 1 x 10^-14

#16
Front (Question)

Buffer solution

Back (Answer)

• solution that resists change in pH • when small quantity of acid or alkali is added

#17
Front (Question)

Ka of buffer solution

Back (Answer)

[salt] x [H+] / [HA]

#18
Front (Question)

Concentrations after dilution

Back (Answer)

(intital volume/total volume) x conc

#19
Front (Question)

End point

Back (Answer)

point where pH changes rapidly

#20
Front (Question)

Equivalence point

Back (Answer)

point where enough acid has been added to react completely with all the base

#21
Front (Question)

Larger Ka, smaller pKa

Back (Answer)

• stronger acid • dissociates more readily in solution • equilibrium lies more to the right

#22
Front (Question)

Limitations of Ka for stronger weak acids

Back (Answer)

• [HA] equilibirum ~ [HA] undissociated • [HA] is bigger than [H+] • Negligible dissociation of H2O

#23
Front (Question)

Buffer explanation

Back (Answer)

• weak acid and soluble salt of weak acid • H+ added, conjugate base reacts, equilibrium shift to the left 3.OH- added, H+ bond, equilibrium shifts to the right

#24
Front (Question)

Carbonic acid hydrogencarbonate

Back (Answer)

CO2(g) +H2O(l) ⇌ H2CO3(aq) ⇌ H+(aq) +HCO3-(aq) • maintains blood pH 7.4 • H+ shifts both equilibrium to the left • OH- shifts equilibrium to the right