EXAM III review session upload

Acid

A substance (neutral molecule or ion) with H in its formula that dissociates in water to yield H3O+ making the solution acidic.

Acid Dissociation

The process where an acid dissociates in water to produce H3O+ and a conjugate base.

Base Ionization

The process where a base ionizes in water to produce OH- and a conjugate acid.

Strong Acid

Acids that completely dissociate in water, characterized by Ka >> 1.

Weak Acid

Acids that slightly dissociate in water, characterized by Ka << 1.

Acid Dissociation Constant (Ka)

The equilibrium constant for the dissociation of an acid in water.

Weak Base

Bases that slightly ionize in water, characterized by Kb << 1.

Base Ionization Constant (Kb)

The equilibrium constant for the ionization of a base in water.

Concentrations of H3O+ and OH-

Represent the concentrations of hydronium ions and hydroxide ions in a solution, respectively.

pH

A measure of the acidity or basicity of a solution, calculated as the negative logarithm of the concentration of hydronium ions in moles per liter.

pOH

A measure of the basicity of a solution, calculated as the negative logarithm of the concentration of hydroxide ions in moles per liter.

Kw

The ion product constant for water, equal to 1.0 × 10^-14 at 25°C.

Strong acids & bases

Acids and bases that undergo complete dissociation in water to produce hydronium ions and anions, or hydroxide ions and cations, respectively.

Acid ionization

The process by which a strong acid dissociates in water to produce hydronium ions and anions.

Base dissociation

The process by which a strong base dissociates in water to produce hydroxide ions and cations.

pH Calculation

The process of determining the pH of a solution by taking the negative logarithm of the concentration of hydronium ions in moles per liter.

pOH Calculation

The process of determining the pOH of a solution by taking the negative logarithm of the concentration of hydroxide ions in moles per liter.

Strong Acid

A substance that completely dissociates into ions in a solution.

Strong Base

A substance that completely dissociates into ions in a solution.

pH

A measure of the acidity or basicity of a solution, calculated as the negative logarithm of the hydrogen ion concentration.

pOH

A measure of the basicity of a solution, calculated as the negative logarithm of the hydroxide ion concentration.

Leveling Effect

The concept that in water, all acids stronger than H3O+ and all bases stronger than OH- appear equally strong.

Weak Acid

A substance that only partially dissociates into ions in a solution.

Weak Base

A substance that only partially dissociates into ions in a solution.

Ka

Acid dissociation constant, a measure of the strength of an acid in solution.

Kb

Base dissociation constant, a measure of the strength of a base in solution.

Weak acids

Acids that do not completely dissociate in water, such as acetic acid (CH3COOH).

Weak bases

Bases that do not completely dissociate in water, such as ammonia (NH3).

Conjugate bases

Anions formed when weak acids donate a proton, such as acetate ion (CH3COO-).

Conjugate acids

Cations formed when weak bases accept a proton, such as ammonium ion (NH4+).

Acid dissociation constant (Ka)

Measure of the strength of a weak acid in water.

Base dissociation constant (Kb)

Measure of the strength of a weak base in water.

Electronegativity

The tendency of an atom to attract a shared pair of electrons towards itself.

Oxoacids

Acids that contain hydrogen, oxygen, and another element, such as sulfuric acid (H2SO4).

Acid strength

Determined by the electronegativity of the central nonmetal and the number of oxygen atoms around it.

Acid strength

The measure of the ability of an acid to donate a proton.

Oxoacids

Acids containing hydrogen, oxygen, and another element.

Electronegativity

The ability of an atom to attract electrons towards itself in a chemical bond.

Conjugate base

The species that remains after an acid has donated a proton.

Polyprotic acids

Acids that can donate more than one proton in successive ionization reactions.

Inductive effect

The ability of atoms to withdraw or donate electron density through sigma bonds.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

Conjugate Pairs

Pairs of acids and bases that differ by a single proton (H+).

Acid-Base Reaction

Chemical reactions where an acid reacts with a base to form a salt and water.

Conjugate Base

The species that remains after an acid has donated a proton.

Conjugate Acid

The species that is formed when a base accepts a proton.

Spectator Ion

Ions that do not participate in the chemical reaction and remain unchanged.

Acid-base reaction equations

Chemical equations that represent the reaction between acids and bases, showing the molecular, total ionic, and net ionic forms.

Molecular equation

A type of chemical equation that shows the complete chemical formulas of reactants and products without indicating the ionic charges.

Net ionic equation

A simplified form of the total ionic equation that only includes the ions that participate in the reaction.

Equilibrium constant (Kc)

A value that indicates the extent of a chemical reaction at equilibrium, with values greater than 1 favoring products and less than 1 favoring reactants.

Weak acid

An acid that only partially dissociates in water, resulting in an equilibrium between the undissociated acid and its ions.

Strong acid

An acid that completely dissociates in water, leading to a high concentration of ions in solution.

Weak acid calculations

Procedures for calculating pH, percent dissociation, equilibrium concentrations, and other parameters related to weak acid solutions.

pH

A measure of the acidity or basicity of a solution, calculated as the negative logarithm of the hydrogen ion concentration.

Equilibrium

A state in which the forward and reverse reactions occur at the same rate, resulting in no net change in the concentrations of reactants and products.

Acetic acid

Chemical formula CH3COOH, a weak acid commonly found in vinegar.

Quadratic equation

An equation of the form ax^2 + bx + c = 0, where x represents an unknown variable and a, b, and c are constants.

Acetic Acid (CH3COOH)

A weak acid commonly found in vinegar, with a chemical formula CH3COOH.

pH

A measure of the acidity or basicity of a solution, calculated as the negative logarithm of the hydrogen ion concentration.

Percentage of Dissociation

The percentage of molecules of a substance that dissociate into ions in a solution.

Equilibrium Constant (Ka)

A measure of the extent of dissociation of a weak acid in a solution.

Weak Base

A base that does not fully dissociate in a solution, such as ammonia (NH3).

Quadratic Equation

An equation of the form ax^2 + bx + c = 0, often used to solve for the concentration of ions in weak base calculations.

Hydroxide Ion (OH-)

A negatively charged ion consisting of one oxygen and one hydrogen atom, often involved in base reactions.

pH

The measure of the acidity or basicity of a solution on a scale of 0 to 14, with 7 being neutral, below 7 being acidic, and above 7 being basic.

Weak Base

A base that does not fully dissociate in solution.

NH3

Ammonia, a weak base commonly used in chemistry.

x

The change in concentration of a species in a chemical equilibrium calculation.

pOH

The negative logarithm of the hydroxide ion concentration in a solution.

Ka

Acid dissociation constant, a measure of the strength of an acid in solution.

H3O+

Hydronium ion, the primary cation present in acidic solutions.

M

Molarity, a measure of the concentration of a solution in moles of solute per liter of solution.

Acid dissociation

The process by which an acid breaks apart into ions when dissolved in water, represented by the equation 𝐻𝐻𝐴𝐴 ⇌ 𝐴𝐴− + 𝐻𝐻3𝑂𝑂+