Chemistry - Acid-Base Reactions
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21 Terms
What is an acid according to the Arrhenius theory?
An acid is a substance that produces hydrogen ions (H⁺) when it dissolves in water.
What is a base according to the Arrhenius theory?
A base is a substance that produces hydroxide ions (OH⁻) when it dissolves in water.
What is a limitation of the Arrhenius theory of acids and bases?
It only applies to aqueous solutions and does not account for reactions in non-aqueous solvents.
What is the Bronsted-Lowry definition of an acid?
proton (H+) donor
What is the Bronsted-Lowry definition of a base?
proton (H+) acceptor
What are conjugate acid-base pairs?
When an acid loses a proton, it forms its conjugate base; when a base accepts a proton, it forms its conjugate acid.
What is an example of a conjugate acid-base pair?
HCℓ is the acid, and Cℓ⁻ is its conjugate base.
What is a strong acid?
A strong acid ionizes completely in water to form a high concentration of H₃O⁺ ions.
Name three strong acids.
Hydrochloric acid (HCl), nitric acid (HNO₃), sulfuric acid (H₂SO₄).
What is a weak acid?
A weak acid ionizes incompletely in water to form a low concentration of H₃O⁺ ions.
Name two examples of weak acids.
Ethanoic acid (CH₃COOH), oxalic acid (C₂H₂O₄).
Strong bases
dissociate completely in water to form a high concentration of OH- ions.
Weak bases
dissociate/ionise incompletely in water to form a low concentration of OH- ions.
Name two strong bases.
Potassium hydroxide (KOH), sodium hydroxide (NaOH).
Concentrated acids/bases
Contain a large amount (number of moles) of acid/base in proportion to the volume of water.
Dilute acids/bases
Contain a small amount (number of moles) of acid/base in proportion to the volume of water.
What is an amphiprotic substance?
a substance that can act as either an acid or a base
Hydrolysis
the reaction of a salt with water.
equivalence point of a titration
The point at which the acid/base has
completely reacted with the base/acid.
Endpoint of a Titration
The point where the indicator changes colour.
Kw
The equilibrium constant for the ionisation of water or the ion product of water or the ionisation constant of water