Solubility Flashcards
Solutions
- Formed when substances dissolve in other substances.
- Homogeneous mixtures.
- Single phase.
- Remain mixed; particles do not settle out.
- Cannot be separated by filtration.
Solvent
- Present in larger amount.
- Dissolves the solute to make the solution.
Solute
- Present in smaller amount.
- Dissolved in the solvent.
Liquid Solutions (Types of Solutions)
- Liquid solvent in which a gas, solid, or liquid is dissolved.
- Ex: carbonated drink.
- Liquid in liquid.
- Ex: antifreeze in water.
- Solid dissolved in a liquid.
- Ex: salt water.
Miscible
- Two liquids mix.
Immiscible
- Two liquids don’t mix.
Solid Solutions (Types of Solutions)
- Alloys: solid mixtures of metals (brass is a mixture of copper and zinc).
Gas Solutions (Types of Solutions)
- Gases dissolved in each other (air is most common example).
Aqueous
- Water is the solvent.
Tincture
- Alcohol is the solvent.
Suspension
- A heterogeneous mixture.
- Particles in the solvent are thousands of times larger than molecules and ion.
- Particles will settle out upon standing.
- Can be separated by filtration.
- Exhibit the Tyndall Effect – the scattering of light in all directions.
Colloid
- Particles are intermediate in size between those of suspension and true solutions.
- Particles do not settle out upon standing.
- Can not be separated by filtration.
- Exhibit the Tyndall Effect.
Emulsion
- Colloidal dispersion of liquids in liquids.
- Emulsifying agent is necessary for maintaining stability.
- Ex: Soap.
Electrolyte
- Dissolves in water to form a solution that conducts electric current.
Non-electrolyte
- Dissolves in water to form a solution that does not conduct electric current.
Surface Area (Factors Affecting the Rate of Solution)
- Increasing the surface area of the solute by crushing speeds up dissolving by increasing the number of collisions between the solute and the solvent surface.
Agitation (Factors Affecting the Rate of Solution)
- Stirring or shaking helps to disperse solute particles, increasing the number of collisions between the solute and the solvent surface.
Heating (Factors Affecting the Rate of Solution)
- Increases the average kinetic energy of the solvent molecules so that collisions between the solvent molecules and the solute are more frequent.
Saturated
- Solution containing all the dissolved solute possible at given conditions of temperature and pressure.
Unsaturated
- Solution containing less dissolved solute that the maximum amount that can be dissolved at given conditions of temperature and solution.
Supersaturated
- Unusual solution containing more dissolved solute than is normally possible at given conditions of temperature and pressure.
Solubility
- A measure of how much solute can dissolve in a given amount of solvent at a specific temperature.
Dilute Solution
- The amount of solute dissolved is small in relation to the amount of solvent present.
- Ex: A teaspoon of salt would dissolve in a gallon of water.
Concentrated Solution
- The amount of solute dissolved is large in relation to the amount of solvent present.
- Ex: A teaspoon of salt would dissolve in a cup of water.
Nature of Solute and Solvent (Factors Affecting Solubility):
- “Like dissolves like.”
- Ex: Polar solutes dissolves in polar solvents; non-polar solutes dissolves in non-polar solvents.
Temperature (Factors Affecting Solubility)
- Generally, increasing the temperature of the solution increases the solubility of a solid solute.
- Increasing the temperature of the solution decreases the solubility of a gaseous solute.
Pressure (Factors Affecting Solubility)
- Only affects the solubility of a gaseous solute.
- Increasing pressure increases solubility.
- Decreasing pressure decreases solubility.
Henry’s Law
- The mass of a gas dissolved in a given volume of liquid is directly proportional to the pressure of the gas.
Molarity
- Expresses solution concentration.
- Molarity = moles of solute/liters of solution
- Molarity, molar, M, and mol/liter all represent the same ratio.
Colligative Properties
- Any of the properties of a solution that change when the concentration of the solution changes.
- Depend on the number of particles dissolved in a given mass of solvent.
Vapor Pressure Depression (Examples of Colligative Properties)
- The lowering of the vapor pressure of a liquid that occurs when substances are dissolved in the liquid.
- Vapor Pressure: the pressure of a vapor in equilibrium with its liquid.
Freezing Point Depression (Examples of Colligative Properties)
- The lowering of the freezing point of a liquid that occurs when substances are dissolved in the liquid.
- Ex: using antifreeze in car radiators and salt on icy roads.
Boiling Point Elevation (Examples of Colligative Properties)
- The raising of the boiling point of a liquid that occurs when substances are dissolved in the liquid.
- Boiling occurs when vapor pressure equals external/atmospheric pressure.
- Ex: antifreeze in a car acts as a coolant in the summer.)
More Examples of Colligative Properties
Color, taste, and density.
