Chemistry

• Solution a homogeneous mixture of two or more substances, its composition are uniformly distributed
• Components of Solution - solute and solvent
• Solute - dissolved substances
• Solvent - dissolving medium
• Types of Solution (Amount of Solute)

  1. Unsaturated Solution
  2. Saturated Solution
  3. Supersaturated Solution
• Unsaturated Solution - more solute dissolves
• Saturated Solution - no more solute dissolves
• Supersaturated Solution - unstable, formation of crystals
• Types of Solution (strength of solute and solvent in a solution)

  1. Hypotonic Solution
  2. Isotonic Solution
  3. Hypertonic Solution
• Isotonic Solution - same strength (saturated solution)
• Hypertonic Solution - more strength (supersaturated solution)
• Hypotonic Solution - less strength (unsaturated solution)
• Energies of Solution Formation

  Low energy : Solute and solvent are compact

  High Energy : Separated solute and compact solvent

  Highest energy : Separated solute and solvent
• Solvation Process - solute particles are surrounded by the solvent particles
• Hydration - water is the solvent
• Concentration amount of substance divided by the total volume of a mixture
• Solubility - amount of solute dissolved in a solvent
• Factors that affect tjhe Solubility of Solute

  1. Nature of Solute
  2. Temperature
• Nature of Solute - “like dissolves like”
• Temperature solubility of solid and liquid is directly proportional to the absolute temperature while gas is inversely proportional
• Factors that Affect the Rate of Dissolving

  1. Stirring or agitation
  2. Heating
  3. Powdering
• Colligative property - does not depend on the kind of matter but instead the amount solute present in a solution
• Types of Colligative Property

  1. Boiling Point Elevation
  2. Freezing Point Depression
  3. Osmotic Pressure
  4. Vapor Pressure
• Boiling point elevation - increase in the boiling point of the solvent due to the addition of solute
• Freezing point depression - the decrease in freezing point of the solvent due to the addition of solute
• Osmotic pressure - pressure applied to pure solvent to prevent it from passing to a solution by the process of osmosis
• Vapor pressure - pressure of vapor in contact with its liquid or solid form
• Boiling point: temperature at which the vapor pressure is equal to the atmospheric pressure
• Freezing point: temperature at which liquid turns to solid
• Osmosis: solvent tends to pass through semipermeable membrane from a less concentration solution to a more concentrated solution to attain equilibrium
• François-Marie Raoult (1887-1888)

  • French chemist showed that the vapor pressure of a solution is equal to the mole fraction of the solvent multiplied by the vapor pressure of the pure liquid (Raoult’s Law)
• Electrolyte solution - contains ions, atoms or molecules that have lost or gained electrons, contains charged particles
• Nonelectrolyte solution - does not conduct electricity due to the absence of charged particles
• Molarity - moles of a solute per liters of a solution
• Molality - total moles of a solute contained in a kilogram of a solvent
• Empedocles

  • Greek Philosopher that proposed the 4 elements and said that the fire element is the primary ancestor concepts on phlogiston and caloric
• Heraclitus

  • Greek Philosopher (500 B.C) said that there are only 3 basic elements
  • Known as “flux and fire” that is “all things are flowing”
• European Scientists who estimated the hotness and coldness of air using thermometer or thermoscope

  • Cornelius Drebbel
  • Robert Fludd
  • Galileo Galilei
  • Santorio Santorio
• Thermochemistry is discovered and developed through the device which is constructed by the Philo of Byzantium and Hero of Alexandria.
• Thermochemistry - concerned with the quantities of heat released and absorbed during chemical reactions