Module 2: ACIDITY AND BASICITY OF ORGANIC COMPOUNDS

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

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Front (Question)

• acids and bases are defined through three main concepts:

Back (Answer)

✓ Arrhenius Theory ✓ Brønsted-Lowry Theory ✓ Lewis electron pair Theory

Front (Question)

BRønsted-Lowry Theory • a “base” is any species that can _________________ • a Brønsted-Lowry base must have at least one lone pair of electron to be able to form bond with a proton

Back (Answer)

accept a proton

Front (Question)

gives the exact strength of a given acid in water

Back (Answer)

Ka (acidity constant)

Front (Question)

ArrHenius Theory • “acid” is any species that can increase the concentration of ______________ in an aqueous solution

Back (Answer)

hydrogen ions (protons) HCl → H+ + Cl–

Front (Question)

ArrHenius Theory • “base” is any species that can increase the concentration of _____________ in an aqueous solution

Back (Answer)

hydroxide ions, OH–, NaOH → Na+ + OH–

Front (Question)

BRønsted-Lowry Theory • an “acid” is any species that can _________________________ • a Brønsted-Lowry acid must have a hydrogen that can dissociate as H+

Back (Answer)

donate a proton (H+)

Front (Question)

___________ react almost completely with water

Back (Answer)

stronger acids (eg. inorganic acids)

Front (Question)

Lewis “electron” pair Theory • an “acid” is a species that can _______________

Back (Answer)

accept a pair of non-bonding electrons

Front (Question)

in a Brønsted-Lowry acid-base reaction a _______________ is the species formed after an acid donates its proton

Back (Answer)

conjugate base

#10

Front (Question)

HCl (aq) + H2O (l) → H3O+(aq) + Cl–(aq) __________ acts as the Brønsted-Lowry acid; __________ is the conjugate base of HCl

Back (Answer)

• HCl • Cl

#11

Front (Question)

react only slightly with water

Back (Answer)

weak acids (eg. acetic acid)

#12

Front (Question)

HCl (aq) + H2O (l) → H3O+(aq) + Cl–(aq) __________ is the Brønsted-Lowry base; ________ is the conjugate acid of the water

Back (Answer)

• H2O • H3O+

#13

Front (Question)

in a Brønsted-Lowry acid-base reaction ____________ is a species formed after the base accepts a proton

Back (Answer)

conjugate acid

#14

Front (Question)

acid strengths are normally given using

Back (Answer)

pKa values (pKa = –log Ka)

#15

Front (Question)

• note that the negative logarithm in the definition of pKa indicates an _____________ between Ka and pKa

Back (Answer)

inverse relationship

#16

Front (Question)

Lewis electron pair Theory • suggest that acids react with bases, ___________, with no change in the oxidation numbers of any atoms

Back (Answer)

sharing a pair of electrons

#17

Front (Question)

Lewis electron pair Theory • a “base” is a species that can ________________

Back (Answer)

donate a pair of non-bonding electrons

#18

Front (Question)

pOH

Back (Answer)

power of hydroxide

#19

Front (Question)

• the Lewis structure of “water” shows that it has a _________________________, therefore acting as the Lewis base

Back (Answer)

non-bonding pairs of valence electrons

#20

Front (Question)

• the reaction between a Lewis acid and a Lewis base gives rise to an _______________

Back (Answer)

acid-base complex or complex ion

#21

Front (Question)

• the “aluminum ion” (Al3+) suggests that it has free orbitals that can ________________________ donated by the water molecules, thereby acting as the Lewis acid

Back (Answer)

accept pairs of non-bonding electrons

#22

Front (Question)

pH means

Back (Answer)

power of hydrogen

#23

Front (Question)

• the acidity and basicity of a substance can be measured in terms of the molar ___________________________ ions, respectively

Back (Answer)

concentration of the hydrogen (H+) or hydroxide (OH–)

#24

Front (Question)

• pOH is defined as the _________________ ion concentration of a substance

Back (Answer)

negative logarithm of the OH–