Introduction to Solutions, Molarity, Acids, Bases, and Titration

Vocabulary practice flashcards covering solutions, colloids, suspensions, molarity calculations, acid-base theories, the pH scale, and titration procedures.

Solution

A homogeneous mixture of two or more substances that has at least one substance dissolved in another, appearing identical throughout and allowing light to pass through.

Solute

The substance present in the smallest amount in a solution that dissolves in the solvent.

Solvent

The substance present in the larger amount in a solution that dissolves the solute.

Suspension

A heterogeneous mixture in which insoluble particles greater than $100\,\text{nm}$ are suspended in a liquid or gas, which settle on their own over time and do not allow light to pass through.

Emulsion

A stable suspension of small droplets of one liquid dispersed in another liquid with which it is immiscible, such as oil and water.

Emulsifying Agent (Emulsifier)

A substance that stabilizes an emulsion by preventing immiscible liquids from separating into distinct layers.

Colloid

A mixture intermediate between a homogeneous solution and a heterogeneous mixture, possessing particle sizes between $1\,\text{nm}$ and $100\,\text{nm}$ that do not settle on their own but settle upon centrifugation.

Tyndall Effect

The scattering of visible light by colloidal or suspended particles as a light beam passes through the mixture.

Brownian Movement

The continuous, random motion of microscopic particles suspended in a fluid or gas resulting from collisions with surrounding atoms or molecules.

Molarity ($M$)

A measure of solute concentration calculated as the number of moles of solute divided by the volume of solution in liters ($\text{Molarity} = \frac{n}{V}$).

Molar Mass

The mass in grams of one mole of a substance, expressed in units of $\text{g}/\text{mol}$.

Polar Covalent Bond (in Water)

A covalent bond between hydrogen and oxygen where oxygen exerts a stronger pull on valence electrons, developing a slight negative charge and leaving hydrogen with a slight positive charge.

Hydrogen Bond (in Water)

An intermolecular attraction formed between the slightly positive hydrogen atom of one water molecule and the slightly negative oxygen atom of another water molecule.

Hydronium Ion ($\text{H}_3\text{O}^+$)

A positively charged ion formed when a water molecule gains a detached hydrogen ion ($\text{H}^+$).

Hydroxide Ion ($\text{OH}^-$)

A negatively charged polyatomic ion formed when a water molecule loses a hydrogen ion ($\text{H}^+$).

pH (Power of Hydrogen)

A scale ranging from $0$ to $14$ measuring the concentration of free hydrogen ions ($\text{H}^+$) or hydronium ions in an aqueous solution, calculated by taking the negative logarithm of the hydrogen ion concentration.

Logarithmic Scale

A nonlinear scale where each equal unit increment increases or decreases the measured quantity by a factor of the logarithm base (such as $10$).

Arrhenius Acid

Any substance that releases hydrogen ions ($\text{H}^+$) when dissolved in water, such as $\text{HCl}$.

Arrhenius Base

Any substance that releases hydroxide ions ($\text{OH}^-$) when dissolved in water, such as $\text{NaOH}$.

Arrhenius Salt

An ionic compound that dissociates in water to release a cation other than $\text{H}^+$ and an anion other than $\text{OH}^-$, such as $\text{NaCl}$.

Brønsted-Lowry Acid

Any substance that acts as a proton ($\text{H}^+$) donor in a chemical reaction.

Brønsted-Lowry Base

Any substance that acts as a proton ($\text{H}^+$) acceptor in a chemical reaction.

Lewis Acid

Any substance that accepts an electron pair.

Lewis Base

Any substance that donates an electron pair.

Acid-Base Indicator

A substance that exhibits a distinct color change in response to changing concentrations of hydrogen ($\text{H}^+$) or hydroxide ($\text{OH}^-$) ions in an aqueous solution.

Universal Indicator

A mixture of multiple chemical indicators that gradually changes color over a wide pH range from $1$ to $14$.

Litmus Paper

A natural pH indicator paper; in acid, blue litmus turns red while red litmus remains red; in base, red litmus turns blue while blue litmus remains blue; in neutral solution, both papers retain their original colors.

Titration

An experimental technique used to calculate the molarity of an unknown solution by reacting a measured volume of an analyte with a titrant of known concentration until neutralization occurs.

Titrant

The solution of known concentration loaded into the buret and dispensed during a titration.

Analyte

The solution of unknown concentration placed in the flask beneath the buret to be analyzed during a titration.