Liquids Test (4/29/16) Flashcards
The most abundant substance in a solution
Solvent
Dissolved substances
Solute
When 2 liquids mix to form homogeneous mixture
Miscible
When liquids separate after mixing
Immiscible
The dissolving process in solid-in-liquid solutions
Solvation
Solvation in water
Hydration
The net energy change during the dissolving process
Enthalpy
The energy goes from the motion of the particles and enters the bonds
Endothermic
The energy exits the bonds and increases the motion, thus the solution heats up
Exothermic
When more solute can still be dissolved
Unsaturated
When a solution contains the maximum amount of a solute
Saturated
When a solution contains more dissolved solute than it does at equilibrium
Supersaturation
When both the solute and solvent occur at the same rate and are balanced
Dynamic equilibrium
When ions are so tightly bound together that you cannot pull them apart
Insoluble
Is a measure of the number of solute particles in a certain volume or mass of the solvent, or of the solution itself. Concentration= amount of solute/ amount of solution (or solvent)
Concentration
Comparison of the solute to the mass of the solution. % by mass= mass of solute/ massof solution x 100%
Percent by mass
Comparison of volume of the solute to the volume of the solution. % by volume= volume of solute/ volume of solution x 100%
Percent by volume
The number of moles of solute per liter of solution. Most common expression of Concentration
Molarity
number of moles of solutes per kilogram of solvent.
Molality
The new properties of a solution that depend upon the number of particles in the solution.
Colligative properties
The change in boiling point
Boiling-point Elevation
1 mole of particles- molecules, atoms, or ions- in 1 kilogram of water elevates the boiling point of water 0.512 C
Molal Boiling-point constant
The change in freezing point
Freezing-point depression
Each solvent has its own that is found by multiplying the molality to find the magnitude
Molal freezing-point constant
The process in which a solvent moves across a semipermeable membrane
Osmosis
The amount of pressure required to prevent osmosis from occurring.
Osmotic Pressure
Mixtures that contain small particles dispersed in a medium.
Colloids
Particles in a colloid (ie. water vapor in a fog)
Dispersed Phase
The medium of a colloid (ie., air for fog)
Dispersing Medium
LCD
Liquid Crystal Displays
A graphical way to summarize the temperature and pressure conditions in which a substance exists as a solid, liquid , or gas.
Phase Diagram
The process of vaporization and condensation can be used to separate mixtures
Distillation
A rapid change between liquid and the gaseous states caused by the application of heat
Boiling
A cooling process that occurs in a non-boiling liquid
Evaporization
The reverse of vaporization- it is the formation of a liquid from its gaseous state.
Condensation
Can occur at or below the boiling- point, and is where molecules break away from the liquid because of their speed
Vaporization
The concave surface that occurs as a result of adhesion for a liquid
Meniscus
A liquids ability to flow
Viscosity
A liquids resistance to flow
Adhesion
The “skin” that forms on the surface of a liquid
Surface tension
The attraction between particles in liquid
Cohesion
Homogeneous mixtures
Solution
