1/16
These flashcards cover key vocabulary and definitions related to acids, bases, and their properties as discussed in the lecture notes.
Name | Mastery | Learn | Test | Matching | Spaced |
---|
No study sessions yet.
Acid (Brønsted-Lowry Definition)
A substance that donates hydrogen ions (H+) to form hydronium ions (H3O+) when dissolved in water.
Base (Brønsted-Lowry Definition)
A substance that forms hydroxide ions (OH-) in water or accepts H+ ions.
Strong Acid
Acids that completely dissociate in water, examples include HCl, HNO3, and H2SO4.
Weak Acid
Acids that do not completely ionize in solution, such as acetic acid and citric acid.
Neutral Substance
A substance that does not ionize, having equal concentrations of H+ and OH- ions.
pH
A measure of the hydrogen ion concentration in a solution, represented as pH = -log [H+].
pOH
A measure of the hydroxide ion concentration in a solution, represented as pOH = -log [OH-].
Titration
A controlled neutralization reaction between an acid and a base, often using an indicator.
Equivalence Point
The point in a titration where the amount of acid equals the amount of base, resulting in complete neutralization.
Polyprotic Acid
An acid that can donate more than one proton (H+), with each dissociation step having a different Ka.
Buffer
A solution composed of a weak acid or base and its conjugate salt, which resists changes in pH.
Common Ion Effect
The phenomenon where the addition of an ion that is part of a solute decreases its solubility in a solution.
Lewis Acid
An electron pair acceptor in the Lewis acid-base definition.
Lewis Base
An electron pair donor in the Lewis acid-base definition.
Ksp (Solubility Product Constant)
An equilibrium constant that reflects the solubility of a slightly soluble ionic solid in a solution.
Henderson-Hasselbalch Equation
An equation used to calculate the pH of a buffer solution based on the concentration of a weak acid and its conjugate base.
Common Use of Buffers
Buffers are used in nature and research to maintain pH stability in biological systems and chemical processes.