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PHYSICAL PROPERTIES OF SOLUTIONS - Coggle Diagram
PHYSICAL PROPERTIES OF SOLUTIONS
Introduction to Solutions
SOLUTION
- A homogenous mixture that is the result of a two or more substances in which the solvent is greater than the amount of the solute. It can be in the form of liquid, solid, and gas.
Unsaturated Solution
- has less than solute than the capacity to dissolve.
Supersaturated Solution
- contains more solute than what is present in a saturated solution and is usually very unstable and sometimes appears as crystals.
Saturated solution
- the solution contains the maximum amount of solute.
TYPES OF SOLUTIONS
GAS + SOLID = SOLID
LIQUID + LIQUID = LIQUID
GAS + LIQUID = LIQUID
SOLID + LIQUID = LIQUID
GAS + GAS = GAS
SOLID + SOLID = SOLID
ENERGY OF SOLUTION FORMATION
SOLUTE- SOLUTE INTERACTION- The separation of solute molecules.
SOLUTE-SOLVENT INTERACTION- The mixture of the solute and solvent.
SOLVENT-SOLVENT INTERACTION - The separation of solvent molecules
ENTHALPY SOLUTION-
refers to the amount of heat that are absorbed or release when the substances go into a solution.
EXOTHERMIC REACTION-
Occurs when the molecules of the solute and solvent react with each other that results to a solution.
ENDOTHERMIC REACTION
- Occurs when the reaction takes in the energy making its surroundings cool down.
EXPAND THE SOLUTE
- each molecules of the solute are separated.
EXPAND THE SOLVENT-
each of the molecules of the solvent are separated.
CONCENTRATION OF SOLUTIONS-
The measurement of the amount of solute that was dissolved in a given amount of solvent.
CONCENTRATED
- has a collectively large of amount of dissolved solute
DILUTE
- has a small amount of dissolved solute
CONCENTRATION UNITS
MOLARITY
- The number of moles of solute in a 1 liter of solution.
MOLALITY
- The number of the moles of a solute dissolved in 1kg of solvent.
PERCENT BY MASS
- The ratio of the solute to the mass of the mass of the solution multiplied by 100 percent.
SOLUBILITY
- It is the maximum amount of a solute that will be dissolved in a given amount of a solvent at a specific temperature.
PRESSURE-
when the pressure of a gas the collision frequency will increase that results to the solubility going up and if the pressure decreases the solubility will go down.
STRUCTURE-
When the difference in molecular structure is greater the lower the mutual solubility will be.
TEMPERATURE-
It affects solubility by increasing the solubility of the substances. If the heat is increased the kinetic energy of the molecules also increases that results to the solvent to dissolve the particles of the solute.
COLLIGATIVE PROPERTIES-
These are the properties that only depend on the number of solute particles in a solution and not on the nature of the solute particles.
OSMOTIC PRESSURE-
This is the pressure required to stop osmosis or the net movement of the solvent molecules through a semipermeable membrane from a pure solvent or dilute solution to a concentrated solution. It is dependent on the molarity of the solution.
FREEZING POINT DEPRESSION-
It occurs when the solute has lower freezing point than the pure solvent. The temperature decreases in the temperature in which the substance freezes. It is dependent on the concentration of the solute.
VAPOR-PRESSURE LOWERING-
When the vapor pressure of a pure solvent is greater than the vapor pressure of the solution that contains a non volatile liquid. It depends on the concentration of the solute in the solution that is expressed by Raoult's law.
BOILING POINT ELEVATION-
It explains what happens when the boiling point of a liquid will be higher when another compound is added that will conclude to the solution having a higher boiling point than a pure solvent. It occurs when a non volatile solute is added to a pure solvent. It is also directly proportional to the molal concentration of solute species.