"In chemistry, concentration is the abundance of a constituent divided by the total volume of a mixture."
The amount of solute present in a given quantity of solution. Can be measured in different ways - molarity, molality, normality, percentage, etc.
Solutions and Solvents: Understanding the concepts of solutions and solvents are the fundamental topics that one needs to know before delving deeper into the concentration of solutions. A solution is a homogeneous mixture of two or more substances, while a solvent is the substance that dissolves the solute to form a solution.
Unit of Concentration: This topic deals with the different methods to express the concentration of a solution, like molarity, molality, normality, percent composition, etc.
Factors Affecting Solubility: Factors like temperature, pressure, and the nature of the solute and solvent affect the solubility of a solution, and this topic sheds light on how these factors have an impact on the concentration of the solution.
Dilution: Dilution is the process of adding more solvent to the solution to decrease its concentration. This topic explains the methods of dilution, and how to calculate the final concentration after the dilution.
Saturated and Unsaturated Solutions: This topic explains the difference between a saturated and unsaturated solution and how they can be distinguished.
Solubility Curves: Solubility curves show how the solubility of a solute varies with changing temperature and pressure. This topic lays emphasis on how to interpret solubility curves.
Colligative Properties: Colligative properties are the properties that depend on the number of solute particles in a solution and not on their nature. The most important colligative properties are vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. This topic explains the principles behind these properties and how they can be measured.
Henry's Law: Henry's law states that the quantity of a gas that dissolves in a liquid is directly proportional to the partial pressure of the gas above the liquid. This topic explains the applications of Henry's law in calculating the concentration of gas in solutions.
Raoult's Law: Raoult's law deals with the partial pressure of the components in a mixture of miscible liquids. It states that the vapor pressure of each component in the solution is equal to its mole fraction times its vapor pressure in the pure state. This topic explains how it can be used to calculate the concentration of each component in the solution.
Ideal and Non-Ideal Solutions: This topic explains the difference between ideal and non-ideal solutions and how to calculate their concentration. Ideal solutions follow Raoult's law, whereas non-ideal solutions deviate from it.
Molarity: Molarity is the measure of the number of moles of solute per liter of solution. It is represented as M.
Molality: Molality is the measure of the number of moles of solute per kilogram of solvent. It is represented as m.
Normality: Normality is the measure of the number of equivalents of solute per liter of solution.
Mass percent: Mass percent is the measure of the mass of solute per 100 grams of solution.
Volume percent: Volume percent is the measure of the volume of solute per 100 milliliters of solution.
Parts per million (ppm): Parts per million is the measure of the number of units of solute per million units of solution.
Parts per billion (ppb): Parts per billion is the measure of the number of units of solute per billion units of solution.
Mole fraction: Mole fraction is the measure of the ratio of the moles of solute to the total number of moles in the solution.
Mole percent: Mole percent is the measure of the percentage of moles of solute in the solution.
Volumetric analysis: Volumetric analysis is the determination of the concentration of a solution by titration.
"Several types of mathematical description can be distinguished: mass concentration, molar concentration, number concentration, and volume concentration."
"The concentration can refer to any kind of chemical mixture, but most frequently refers to solutes and solvents in solutions."
"The molar (amount) concentration has variants, such as normal concentration and osmotic concentration."
"Dilution is reduction of concentration, e.g. by adding solvent to a solution."
"The verb to concentrate means to increase concentration, the opposite of dilute."
"The abundance of a constituent divided by the total volume of a mixture."
"Molar concentration measures the amount of a constituent per unit volume of the mixture."
"Number concentration refers to the number of particles of a constituent per unit volume of the mixture."
"Volume concentration measures the volume of the constituent per unit volume of the mixture."
"No, the concentration can refer to any kind of chemical mixture."
"Dilution involves adding solvent to a solution to reduce the concentration."
"Normal concentration is a variant of molar concentration."
"Osmotic concentration is another variant of molar concentration."
"The verb to concentrate means to increase concentration."
"The opposite of dilute, reduction of concentration, can be achieved by adding solvent to a solution."
"By dividing the abundance of a constituent by the total volume of a mixture."
"Molar concentration relates the amount of a substance to the volume of the mixture."
"Number concentration indicates the number of particles of a constituent in a given volume of the mixture."
"Volume concentration reflects the volume of a constituent in relation to the overall volume of the mixture."