Reviewer in Chem

Cards (46)

  • Temperature
    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 solution with 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 cannot dissolve 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 not capable of dissolving
  • Aqueous solution

    • A solute is dissolved in water
  • Non-aqueous solution

    • A solute is dissolved in a solvent other than water
  • 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