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April 20, 2023 2
Arrhenius Definition of Acids & Bases
• Acids release H+ ions when dissolved in water.– HCl(g) H+(aq) + Cl-(aq)
• Bases release OH- ions when dissolved in water.– NaOH(s) Na+ (aq) + OH- (aq)
April 20, 2023 5
Limitations of Arrhenius Concept: Restricted to aqueous solutions
• More general definition offered independently by Johannes Bronsted and Thomas Lowry (1923)
• Focuses on the transfer of H+ ions from one substance to another
• An H+ ion is simply a proton with no surrounding valence electrons; interacts strongly with nonbonding electons pairs of water molecules to form hydronium ions, H3O+ (aq)
April 20, 2023 11
Bronsted-Lowry Acids & Bases
• An acid is a substance that can donate a proton to another substance.
• A base is a substance that can accept a proton.
• A tug-of-war between an acid & base for proton (in the form of H+)
• Because the emphasis is on proton transfer, can be applied to non-aqueous reactions, too.
April 20, 2023 12
• A substance can function as an ACID only if another substance simultaneously behaves as a BASE.
• Acid – must have a H atom to lose as an H+ ion• Base – must have a nonbonding pair of
electrons to bind to H+ ion.
April 20, 2023 13
Stupid Sports Analogy…
Acids are the quarterback, throwing away a PROTON (football) Bases are the receivers, catching the
PROTON, (football)
April 20, 2023 14
Conjugate Acid-Base Pairs
• Consider a reversible reaction:
• HX (aq) + H2O X- (aq) + H3O+ (aq)
April 20, 2023 15
• When reaction is reversed, X- acts as base and H3O+ acts as acid.
• HX (aq) + H2O(l) X- (aq) + H3O+ (aq) • Every acid has a conjugate base, formed by
removing a proton from the acid.HX (aq) acidX- (aq) conjugate base
H2O (l) baseH3O+ (aq) conjugate acid