Chapter 15 Flashcards
(85 cards)
Vital to biological systems normal function
Acid-base balance
Regulated by the reversible chemical reactions
The amount of acid-base in a system
Arrhenius acid
Dissociate in water to produce H+
Dissociate in water to produce H+
Arrhenius acid
Arrhenius base
Ionizes or dissociates in water to produce OH-
Ionizes or dissociates in water to produce OH-
Arrhenius base
Arrhenius acid-base reactions
Cation from base plus anion of acid forms salt in water (from OH + H)
Cation from base plus anion of acid forms salt in water (from OH + H)
Arrhenius acid-base reaction
Problems with Arrhenius theory
Doesn’t explain basicity/acidity of molecules or compounds lacking OH- or those lacking H+
Can’t explain acid-base reactions that take place outside aqueous solution
Brønsted-Lowry acid
Proton (H+) donors
Proton (H+) donors
Brønsted-Lowry acid
Brønsted-Lowry base
Proton (H+) acceptors
Proton (H+) acceptors
Brønsted-Lowry base
Amphoteric substance
Acts as an acid or a base, water is most common
Acts as an acid or a base, water is most common
Amphoteric substance
Nonmetal oxides
Form acids when placed in water
Ex: SO2, SO3, CO2 (all gases)
Conjugate acid-base pairs
Exist on the other side of equilibrium, opposite of left hand side, only possible in Brønsted-Lowery theory, not Arrhenius
Conjugate acid
From original base, add H+
From original base, add H+
Conjugate acid
Conjugate base
From original acid, minus H+
From original acid, minus H+
Conjugate base
Strong acid
Strong electrolyte, complete ionization, more willing to donate H+
Strong acids
3 binary, 3 oxy acids
5 monoprotic, 1diprotic
Binary acid
Consists of only 2 elements