Unit 8: Study Guide for Acid-Base Fundamentals
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25 Terms
Arrhenius Acid
A substance that increases the concentration of hydrogen ions (H+) in aqueous solution.
Arrhenius Base
A substance that increases the concentration of hydroxide ions (OH-) in aqueous solution.
Brønsted-Lowry Acid
A proton (H+) donor.
Brønsted-Lowry Base
A proton (H+) acceptor.
Conjugate Acid-Base Pair
The acid and base that transform into each other by the loss or gain of a proton.
Amphiprotic Species
A substance that can act as either an acid or a base depending on the reaction.
Autoionization of Water
The process in which water acts as both an acid and a base to produce hydronium and hydroxide ions.
Ion-Product Constant (Kw)
At 25°C, Kw = [H3O+][OH-] = 1.0 x 10^-14.
pH Scale
A logarithmic scale used to specify the acidity or basicity of a solution.
Strong Electrolytes
Substances that dissociate completely in water.
Strong Acids
Acids that completely ionize in solution, such as HCl, HNO3, and H2SO4.
Strong Bases
Bases that completely dissociate in aqueous solution, typically hydroxides of Group 1 and some Group 2 metals.
Dissociation Constant (Ka)
An equilibrium constant that measures the strength of a weak acid.
Dissociation Constant (Kb)
An equilibrium constant that measures the strength of a weak base.
Percent Ionization
The ratio of the concentration of ionized acid to the initial concentration of acid, expressed as a percentage.
Binary Acids
Acids composed of two elements, typically hydrogen and a nonmetal.
Oxyacids
Acids that contain hydrogen, oxygen, and a central nonmetal.
Electronegativity
A measure of the tendency of an atom to attract a bonding pair of electrons.
Inductive Effect
The effect on the acidity of a compound due to electronegative atoms pulling electron density away from the O-H bond.
Strong Acid Examples
Examples include HCl, HBr, HI, HNO3, H2SO4, HClO4.
Strong Base Examples
Examples include NaOH, KOH, Ba(OH)2, Sr(OH)2.
pOH
A measure of the hydroxide ion concentration of a solution, calculated as pOH = -log[OH-].
pH + pOH Relationship
At 25°C, pH + pOH = 14.00.
Stoichiometry of Bases
The consideration that some Group 2 hydroxides produce more than one hydroxide ion when dissolved.
Temperature Dependency of Kw
Kw increases with a rise in temperature, affecting the pH of neutral water.
