Acid-Base Theory and Titrations

This set of flashcards covers key terms and concepts related to acid-base theory, titrations, and solubility equilibria based on the notes from the lecture.

Acid

A substance that donates protons (H+) in an aqueous solution.

Base

A substance that accepts protons (H+) or donates hydroxide ions (OH−) in an aqueous solution.

Arrhenius Acid

Produces H+ in an aqueous solution.

Arrhenius Base

Produces OH- in an aqueous solution.

Neutralization Reaction

A chemical reaction between an acid and a base that produces a salt and water.

pH scale

A measure of how acidic or basic a solution is, ranging from 0 (acidic) to 14 (basic). A pH of 7 is considered neutral.

Hydronium Ion (H3O+)

A water molecule (H2O) that has accepted an additional proton (H+).

Common Ion Effect

The decrease in solubility of a salt when a common ion is added to the solution.

Conjugate Acid

The species produced when a base accepts a proton.

Conjugate Base

The species produced when an acid donates a proton.

Lewis Acid

An electron pair acceptor.

Lewis Base

An electron pair donor.

Buffer

A solution that resists changes in pH upon the addition of small amounts of acid or base.

Henderson-Hasselbalch Equation

A formula for calculating the pH of a buffer solution: pH = pKa + log([A−]/[HA]).

Ka (Acid Dissociation Constant)

A measure of the strength of an acid in solution.

Ksp (Solubility Product Constant)

An equilibrium constant that applies to the solubility of ionic compounds.

Titration

A quantitative analytical method used to determine the concentration of a solute by reacting it with a standard solution.

Equivalence Point

The point in a titration at which the number of moles of acid equals the number of moles of base.

Indicator

A substance that changes color at a specific pH range, used to determine the endpoint of a titration.

Amphoteric Substance

A substance that can act as both an acid and a base.

Dissociation

The process by which a compound breaks apart into its individual ions.

Molar Solubility

The maximum amount of solute that can dissolve in a liter of solution.

Ion Product (Q)

The product of the concentrations of the ions in a solution, used to predict if a precipitate will form.

Strong Acid

An acid that completely ionizes in aqueous solution.

Weak Acid

An acid that partially ionizes in aqueous solution.

Strong Base

A base that completely dissociates in aqueous solution.

Weak Base

A base that partially dissociates in aqueous solution.

pKa

The negative logarithm of the acid dissociation constant (Ka); a lower pKa value indicates a stronger acid.

Dissociation Constant (Kb)

The equilibrium constant for the dissociation of a base.

Polyprotic Acid

An acid that can donate more than one proton (H+).

Buffer Capacity

The amount of acid or base a buffer can neutralize before its pH changes significantly.

Base Ionization Constant

The equilibrium constant for the ionization of a base.

Saturated Solution

A solution that contains the maximum amount of solute that can dissolve at a given temperature.

Unsaturated Solution

A solution that can still dissolve more solute at a given temperature.

Supersaturated Solution

A solution that contains more solute than is typically soluble at a given temperature.

Electrophile

A species that accepts an electron pair to form a covalent bond.

Nucleophile

A species that donates an electron pair to form a covalent bond.

Precipitate

A solid formed from a solution during a chemical reaction.

pOH

The negative logarithm of the hydroxide ion concentration; pH + pOH = 14.

Hydroxide Ion (OH−)

A negatively charged ion formed when a base dissolves in water.

Ionic Product

The product of the concentrations of the ions involved in a solubility equilibrium.

Autoionization of Water

The reaction in which water ionizes to produce H3O+ and OH−.

Solubility Equilibrium

The dynamic equilibrium between the dissolved and undissolved forms of a solute.

Common Anion

An ion that is shared between two solutions, affecting the solubility of a salt.

Electrolyte

A substance that dissociates into ions in solution and can conduct electricity.

Chemical Equilibrium

A state where the concentrations of reactants and products remain constant over time.

Le Chatelier's Principle

When a system at equilibrium is disturbed, the system shifts to counteract the disturbance.

Kf (Formation Constant)

The equilibrium constant for the formation of a complex ion.

Ksp (Solubility Product Constant)

An equilibrium constant that applies to ionic compounds that are sparingly soluble.

Solubility Product Expression

A mathematical expression used to describe the solubility of a sparingly soluble salt.

Acidic Solutions

Solutions that have a pH less than 7; more concentrated in hydronium ions.

Basic Solutions

Solutions that have a pH greater than 7; more concentrated in hydroxide ions.

Chemical Reaction

The process which leads to the transformation of one set of chemical substances to another.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Spectator Ion

An ion that does not participate in a chemical reaction and remains in solution.

Hydrolysis

The reaction of a substance with water, resulting in the formation of ions.

Cation

A positively charged ion.

Anion

A negatively charged ion.

Ion Exchange

The reversible interchange of ions between the solid phase and the liquid phase.

Buffer Range

The pH range over which a buffer effectively resists changes in pH.

Precipitation Reaction

A reaction in which dissolved substances form an insoluble solid.

Solubility Curve

A graph that shows how the solubility of a substance changes with temperature.

Lone Pair

A pair of valence electrons that are not shared with another atom.

Redox Reaction

A reaction involving the transfer of electrons between two chemical species.

Catalyst

A substance that speeds up a chemical reaction without being consumed in the process.

Saturation

The maximum concentration of solute that can be dissolved in a solvent at a given temperature.

Diprotic Acid

An acid that can donate two protons (H+ ions).

Triprotic Acid

An acid that can donate three protons (H+ ions).

Solubility Product Constant Expression

Ksp = [Cation][Anion]^n, where n is the number of moles of anion produced per mole of solid.

Salt Hydrolysis

The reaction of a salt with water to produce an acidic or basic solution.

Weak Electrolyte

A substance that partially ionizes in solution producing fewer ions.

Strong Electrolyte

A substance that completely dissociates into ions in solution.