Test 12 Flashcards
Homogeneous mixtures of variable composition in a single phase
Solutions
The most abundant substance in a solution
Solvent
Dissolved substances in a solution
Solute
A solution containing mercury
Amalgam
What is the only permanent gas solution at ordinary pressures
Why
Gaseous solvents dissolve and gaseous solutes.
Gases cannot dissolve liquid or solid particles because gas particles are so much smaller than liquid or solid particles
What is the governing principle in solutions
Like dissolves like
What is the maximum amount of a solute that can dissolve in a specific solvent under specific conditions, such as temperature and pressure
Solubility
What accounts for the different solubility
The strength of ionic attractions within compounds
Are supersaturated solution stable
No
What can affect the frequency of collisions with solvent particles
Temperature, stirring, and the amount of surface area of the solute exposed to the solvent
The escape of a gas from a liquid gas solution
Effervescence
What are the most common ways to express concentration
Percent by mass, molarity, and molality
What is the formula for percent by mass
Percent by mass =
(mass of solute/mass of solution) x100%
What is the formula for percent by volume
Percent by volume = (volume of solute/volume of solution) x100%
What’s the formula for molarity
Molarity (M) = mol solute/L solution
What four things change because of the presence of solutes instead of just a pure solvent
Freezing points
Boiling points
Vapor pressures
Osmotic pressures
The more concentrated a solution is, the___ the boiling point elevation will be
Greater
Solutions freeze at___temperatures than their pure solvents
Lower
What is osmotic pressure of a solution
The amount of pressure required to prevent osmosis from occurring
Why is osmotic pressure of a solution a colligative property
Because it depends on the number of particles in a solution
Why should the solution surrounding a cell be kept at the same osmotic pressure as a solution inside the cell
If the equilibrium is disturbed, water could leave the cell in sufficient quantities and cause dehydration
OR water could enter the cell and cause the membrane to burst
What happens if a cell is placed in a hypertonic solution
Water will flow out of the cell into the surrounding solution
What happens if a cell is placed in a hypotonic solution
Water will flow into the cell, causing it to swell and possibly burst
What is isotonic
When concentrations on both sides of the membrane are equal
Mixtures that contain larger particles that will eventually settle out of the mixture
Suspension
Fog is a__
Colloid
What phases can a colloid exist in
Solids, liquids, and gases
Can a gas/gas colloid exist why or why not
No, they are always solutions
List three types of colloids
Foams
Aerosols
Gels
Completely describe the three steps involved in practical water treatment
1- pathogens are killed by chlorinating the water with chlorine dioxide or similar compounds
2- other compounds are added to clump impurities together causing coagulation
3- The water is passed through a filter under pressure to quickly remove impurities
Gas/gas is
Only a solution
What keeps particles smaller than 1000 nm in colloids from setting out
Intermolecular collisions
M=
Mol/L
K(b)
Molal boiling point
Delta T(b)
The CHANGE in boiling point NOT The new boiling point!
ADD original to get new one
Pertaining to two liquids that are not soluble in each other
Immiscible
The process in which solvent particles surround and interact with solutes
The dissolving process in
solid-in-liquid solutions
Solvation
A type of solvation in which water molecules surrounded interact with solute particles
Hydration
A type of solvation in which an ionic compound forms ions when it dissolves in a solvent
Dissociation
A type of solvation in which a covalent compound forms ions when it dissolves in a solvent
Ionization
The inability of a solute to dissolve in a certain solvent
Insoluble
A chemical equilibrium in which two or more opposing events occur at the same rate that results in no net change
Dynamic equilibrium
A quantitative measure of concentration equal to the number of moles of solution per kilogram of solvent
Molality (m)
A physical property of a solution that depends only on the number of solute particles present without regard to type
Colligative property
A number that relates the change in boiling point of a particle solvent to the concentration of solute particles
Molal boiling point constant K(b)
The diffusion of pure solvent molecules, such as water, through a semi permeable membrane
Osmosis
A mixture of small particles that remain dispersed in a medium
Colloid
In a colloidal mixture, the phase in which the particles are spread out
Dispersed phase
The scattering of light by particles in a colloid
The Tyndall effect
The random, chaotic movements of microscopic particles
Brownian motion
