Acids and Bases
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A comprehensive set of vocabulary flashcards covering key concepts related to acids, bases, and their reactions in solutions.
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30 Terms
Acid
A species that dissociates in water to produce hydrogen ions (H+) and forms hydronium ions (H3O+).
Base
A species that dissociates in water to produce hydroxide ions (OH-).
Acid-Base Reaction
A reaction that involves the transfer of a hydrogen ion (H+) from one reactant to another.
Brønsted-Lowry Acid
A substance that donates a proton (H+).
Brønsted-Lowry Base
A substance that accepts a proton (H+).
Conjugate Acid
The species formed when a base accepts a proton.
Conjugate Base
The species formed when an acid donates a proton.
pH Scale
A scale that indicates the acidity or basicity of a solution, ranging from 0 (very acidic) to 14 (very basic).
Strong Acid
An acid that dissociates completely in water.
Weak Acid
An acid that only partially dissociates in water.
Ion Product of Water (Kw)
The equilibrium constant for the autoionization of water, which equals [H3O+][OH-] and is typically 1.0 x 10^-14 at 25°C.
Buffer
A solution that resists changes in pH when small amounts of acid or base are added.
Titration
A technique used to determine the concentration of an acid or base by reacting it with a standard solution of base or acid.
Henderson-Hasselbalch Equation
An equation that relates pH, pKa, and the concentration of an acid and its conjugate base.
pKa
The negative logarithm of the acid dissociation constant (Ka), indicating the strength of an acid.
Polyprotic Acid
An acid that can donate more than one proton per molecule.
Electrolyte
A substance that, when dissolved in water, conducts electricity.
Autoionization
The reaction in which water dissociates into hydrogen ions and hydroxide ions.
Conjugate Acid-Base Pair
An acid and base that differ by one proton.
Acid Dissociation Constant (Ka)
The equilibrium constant for an acid's dissociation in water.
Base Ionization Constant (Kb)
The equilibrium constant for a weak base's ionization in water.
The Seven Strong Acids
The strong acids include HCl, HBr, HI, HNO3, H2SO4, HClO3, and HClO4.
The Seven Strong Bases
Base are soluble strong hydroxides: NaOH, KOH, and Ba(OH)2.
Indicator
A chemical that changes color in response to changes in pH.
Common Ion Effect
The decrease in solubility of a salt when a common ion is added.
Amphoteric
Substances that can act as both acids and bases, such as water.
What is a buffer?
a solution that resists changes in pH when small amounts of acid or base are added.
How do buffers work?
work by using weak acids and their conjugate bases to neutralize added acids or bases, maintaining the pH within a narrow range.
What is titration?
a technique in which a solution of known concentration is used to determine the concentration of another solution.
How does titration work?
titrant is gradually added to a sample until the reaction reaches its endpoint, indicated by a color change or a pH indicator.