Chemistry Lecture: Equilibrium, Solutions, Acids, Bases, and Colligative Properties

Flashcards covering chemical equilibrium, solution properties, molarity calculations, acid-base theories, and colligative properties based on lecture slides 1-128.

Equilibrium

A state of chemical balance between the products and reactants in a chemical reaction where the rates of the forward and backward reactions are equal.

Equilibrium Arrow ($\leftrightarrow$)

A double-sided arrow used to represent equilibrium in a chemical reaction.

Le Chatelier’s Principle

States that a chemical reaction will shift toward the reactants or products to compensate for an external change to restore equilibrium.

Solution

A homogeneous mixture of two or more unique substances where the parts of the mixture cannot be distinguished.

Alloy

A solution of two metals.

Solute

The substance being dissolved into a solution, typically the smaller substance.

Solvent

The substance dissolving the solute into the solution, typically the larger substance.

Universal Solvent

A title given to water ($H_2O$) because of its prevalence in dissolving substances.

Solubility

The ability for the solute to dissolve into the solvent.

Solvable

A term describing a solute that can be dissolved in the solvent.

Insoluble

A term describing a solute that cannot dissolve in the solvent.

Solvation

The process of surrounding the solute particles with the solvent particles.

Hydration

The chemical term for solvation specifically when water ($H_2O$) is the solvent.

Cation

A positively charged ion, such as $Na^{+}$.

Anion

A negatively charged ion, such as $Cl^{-}$.

Polarity

The sharing of electrons in a compound; can be even (non-polar) or uneven (polar).

Non-Polar Compound

A compound characterized by the even sharing of electrons.

Polar Compound

A compound characterized by the uneven sharing of electrons.

Molarity ($M$)

The concentration of a solution calculated as $\frac{\text{moles of solute}}{\text{L solution}}$.

Dilution

The process of making a solution weaker by adding more solvent.

Concentrate

The process of making a solution stronger by adding more solute.

Acid

A substance with a high amount of hydrogen ions ($H^{+}$) or protons; properties include sour taste and reacting with metals to form hydrogen gas ($H_2$).

Hydronium Ion ($H_3O^{+}$)

An ion given off by acids when in aqueous solutions.

Base

A substance with a high amount of hydroxide ions ($OH^{-}$); properties include bitter taste, filmy feel, and being corrosive.

Corrosive

The ability to break down or dissolve certain substances.

Arrhenius Model

An acid-base theory defining acids as substances that give a hydrogen ion ($H^{+}$) and bases as substances that give up a hydroxide ion ($OH^{-}$).

Bronsted-Lowry Model

An acid-base theory defining acids as proton ($H^{+}$) donors and bases as proton ($H^{+}$) acceptors.

Amphoteric

A substance, like water ($H_2O$), that can act as both an acid and a base.

Neutralization Reaction

A chemical reaction where an acid and a base react to form a salt and water.

Salt

An ionic bond with a metal and non-metal, excluding oxygen.

Dissociates

The process where a compound splits into its ion forms, such as $HCl \rightarrow H^{+} + Cl^{-}$.

Binary Acid

An acid made when hydrogen forms a bond with a non-metal element, named with the prefix 'hydro-.'

Tertiary Acid

An acid made when hydrogen forms a bond with a negative polyatomic ion; these names do not use a prefix.

Conjugate Acid

A base that has received a hydrogen ion (proton) and now wants to give the proton away.

Conjugate Base

An acid that has donated a hydrogen ion (proton) and now wants to take the proton back.

Colligative Properties

Properties of solutions affected by the amount of solute present, but not the identity of the solute.

Vapor Pressure Lowering

The effect where adding solute keeps solvent particles from turning into vapor gas at the surface.

Boiling Point Elevation

The increase in the boiling point of a solution compared to the pure solvent due to the amount of solute.

Molality ($m$)

A concentration comparing the moles of solute to the mass ($kg$) of the solution; used because mass remains constant regardless of pressure and temperature changes.

Freezing Point Depression

The difference in freezing point between a pure solvent and a solution containing solute.

Osmosis

The movement of particles from an area of high to low concentration across a semi-permeable membrane.

Osmotic Pressure

Additional pressure resulting from the movement of water from one area to another.

pH Scale

A scale ranging from 0 to 14 used to determine the strength of an acid or base.

Litmus Paper

Test paper that changes color to show whether a solution is an acid (red) or a base (blue).

Indicator

A substance that has a specific color for acidic and basic substances, such as pH paper or Universal Indicator.