solutions Flashcards
mixture
two or more substances physically combined
homogenous
a mixture that is uniform throughout (solution)
heterogenenous
a mixture that is not uniform throughout
soluble
a substance that is dissolved (aqueous)
insoluble
a substance that does not dissolve (a precipitate)
solution
a homogenous mixture that contains a solute that is fully dissolved in a solvent
solution examples
steel, sugar water, air
solute
substance that dissolves in .a solvent
solvent
substance that dissolves a solute
what does the solvent do in a solution
pulls the solute apart and distributes the particles
saturated
solution that can not dissolve any more solute at a given temperature and pressure
unsaturated
a solution that can dissolve more solute at a given temperature and pressure
supersaturated
a solution in which excess solute precipitates out of the solution at a given temperature and pressure q
what is solubility
maximum amount of a solute that will dissolve in a given amount of solvent at a specific temperature and pressure
precipitate
forms if the substance is insoluble
substance is aqueous
if the substance is soluble
non polar covalent bond
bond in which electrons are equally shared
polar covalent bond
electrons not equally shared
-one element is more electronegative, so electrons more attracted to more electronegative element, creating a partial charge
nonpolar dissolves in
nonpolar
polar dissolves in
polar
miscible
two liquids are soluble in each other
immiscible
two liquids are not soluble in each other
what factors affect the rate of solubility
surface area
temperature
pressure of gas
how does temp affect solubility
- increased temp of a solid to increase solubility
- decrease temp of a liquid or gas to increase solubility
how does surface area affect solubility
agitation (stirring) allows smaller particles to contact the solute
how does pressure of a gas increase solubility
increasing the pressure of a gas increases the solubility
what does a solubility graph show
shows how temperature affects solubility
indentify the species of the graph
unsaturated: below the curve
saturated: on the curve
supersaturated: above the curve
what is a stock solution
- called standard solution
- solution whose concentration is known
concentrated
if a solute contains a large amount of product
dilute
if it contains a small amount of solute
concentration
a measure of how much solute is dissolved in a solvent
molarity
measure of concentration of a solute
unit M or moles/litres
molarity formula
moles of a solute /litres of solution
dilution
used to dilute a stock solution
remember significant figures
dilution formula
m1 x v1 = m2 x v2
how to prepare a standard solution
- mass the solute
- add the solute and deionized water
- swirl solution and dissolve solute
- add deionized water to the mark
water
- the most common solvent
- H and O held together by polar covalent bonds
charges of water
- partial positive charge around both hydrogens
- partial negative charge around the oxygen
shape of water
bent shape because the two unshared electrons pairs require more space
what are the properties of water (non -high ones)
- unequal distribution of electrons
- soluble because of polarity
- dissolve nonpolar molecules like alcohols and sugars
properties of water (high ones)
- high heat of vaporization
- high specific heat
- high cohesive forces
- high adhesive forces
heat of vaporization
heat required to change 1 g of H2O to gas
specific heat
heat required to change 1 g of H2O to 1 degree
cohesive force
attraction between like molecules
adhesive forces
attraction between unlike molecules
solid water
arranged in orderly, open framework result in a less dense substance
liquid water
move and allow opposing forces to come between the molecules, results in a denser substance
intramolecular forces
forces that hold atoms together within a molecule
stronger than intermolecular forces
types of intramolecular forces
ionic bond
covalent bond
intermolecular forces
forces that hold two or more molecules together
types of intermolecular forces
dipole-dipole
hydrogen bond
london dispersion force
dipole-dipole
an attraction between oppositely charger regions of polar molecules
hydrogen bond
a type of dipole-dipole force in which a H in one molecule bonds with a F, O , or N in another molecule (is very strong)
landon dispersion force
type of van der Waal force that occurs between non polar molecules in which electrons shift positions (very weak)
what is an electrolyte
an ionic compound whose solution conducts electricity because it dissociates
strong electrolyte
a strong acid and strong base, completely dissociates
weak electrolyte
weak acid and weak base, does not completely dissociate
non electrolyte
a compound whose solution does not conduct electricity because it does not dissociate
what dissociate
ionic compounds, breaks into the individual atoms
does not dissociate
does not break into individual atoms, breaks into individual molecules
examples of non electrolytes
water, sugar, alcohol
is water polar
yes
