Measure of the average kinetic energy of the atoms or molecules in the system
Solubility
The ability of a substance, the solute, to form a solutionwith another substance, the solvent
Solvent
A substance that dissolves to form a solution
Solute
A substance that dissolves in a solvent
Solution
A mixture of a solute and a solvent
Soluble
A material that can dissolve in a solvent
Insoluble
A material that cannotdissolve in a solvent
Types of solution
Supersaturated solution
Unsaturated solution
Saturated solution
Aqueous solution
Non-aqueous solution
Supersaturated solution
Comprises a large amount of solute at a temperature wherein it will be reduced
Unsaturated solution
In which a solvent is capable of dissolving
Saturated solution
In which a solvent is notcapable of dissolving
Aqueous solution
A solute is dissolved in water
Non-aqueous solution
A solute is dissolved in a solventotherthanwater
Factors affecting solubility
Nature of the solvent and solute
Pressure
Temperature
Amount of solvent
Manner of stirring
Presence of other solutes
Particle size
Type of solvent
Nature of the solvent and solute
Like dissolves like
Increase in pressure
Typically increases the solubility of a gas in a liquid (solid and liquid are not affected)
Raising the temperature
Will increase the solubility of a solute in a solvent
Amount of solvent
Plays a crucial role in determining how much solute can dissolve
Manner of stirring
Stirring a solution increases the solute's contact with the solvent
Presence of other solutes
One solute can enhance or inhibit the solubility of another solute through various interactions
Particle size
Smaller particles have a smaller surface area
Type of solvent
The choice of solvent plays a crucial role in determining how well a solute dissolves
Endothermic and exothermic processes
Endothermic process
Exothermic process
Endothermic process
Chemical or physical reactions that absorb energy from the surroundings
Endothermic process
Photosynthesis
Dissolution of ammonium nitrate
Exothermic process
Chemical or physical reactions that release energy in the form of heat to the surroundings
Exothermic process
Burning of sugar
Water and calcium chloride
First Law of Thermodynamics
Also known as the law of energy conservation, states that energy cannot be created or destroyed, only transformed
The First Law of Thermodynamics states that the universe's total energy is constant
Thermodynamics
The study of the relation between heat, work, temperature, and energy
Rudolf Clausius and William Thomson (Kelvin) developed the First Law of Thermodynamics
Hess's Law
A fundamental principle in chemistry that states that the total enthalpy change during a chemical reaction remains the same
Hess's Law
Based on the concept that enthalpy is a state function, it depends only on the initial and final states of a system
Allows us to calculate the overall change in enthalpy by simply summing up the changes
Enthalpy
A thermodynamic quantity that represents the total heat content of a system, often used to describe the heat flow in a constant pressure
Enthalpy of formation
The enthalpy change that occurs when one mole of a compound is formed from its elements in their standard states, the enthalpy change that occurs in a chemical reaction
Molarity
The concentration of a solution expressed as moles of solute per liter of solution
Molar mass
Mass of one mole of a substance and is expressed in grams per mole (g/mol)
Stoichiometry
A branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions
Colligative properties
Freezing point depression
Boiling point elevation
Vapor pressure lowering
Osmotic pressure
Colligative properties
Physical changes that result by adding solute to a solvent