unit 4 Flashcards
solution
Homogeneous mixture of two or more substances
Aqueous solution
A solution in which water is the solvent
solvent
The substance that does the dissolving
solute
The substance that is dissolved
concentration
ratio of solute to solution or solvent
concentrated solution
Solution with large quantity of solute in solvent
dilute solution
solution with small quantity of solute in solvent
saturated solution
no more solute can dissolve
supersaturated solution
More than maximum amount of solute is present, if one more crystal is added, the solute will precipitate out
unsaturated solution
A solution that is not yet saturated
solubility
The amount of solute which will be dissolved in a given volume of solvent at a specific temperature
insoluble
Solubility less than 0.1 g in 100 mL
Slightly soluble
Solubility between 0.1 g and 1 g in 100 mL
soluble
Solubility is 1 g or greater in 100 mL
dissociation
processed by which compounds separate into smaller molecules when in water
ex. CaCl2 —> Ca2+ (aq) + 2Cl - (aq)
ionization
The formation of ions from polar covalent compounds when placed in water
miscible
substances able to combine with each other in any proportion
immiscible
substance is not able to combine with each other
why water is the universal solvent
1) polarity
2) hydrogen bonding (water molecule is bent)
3) small molecule
generalization of solubility
solids -high solubility at high temps
gases- high solubility at low temps
liquids- cannot generalize
factors that affect solubility
1) increase surface area (large solids are harder to dissolve)
2) agitation (stir the solution)
3) increase temperature of solution
how do you solve for solubility
g/mL = g/mL
then cross multiply
solving for concentration
c = n/v
*volume must be in litres
1) find MM of solution
2) find moles using n= m/MM
3) find c
how else can you represent concentration
square brackets
what are the two ways to prepare a solution
from a solid:
n = c x v
1) find n
2) find m
or dilution:
C1V1 = C2V2
what is a total ionic equation
includes every ion
what is a net ionic equation
simplified version
what are spectator ions
does not change chemical reaction
what does pH stand for
potential of hydrogen
what are the pH levels
pH 7 is neutral
pH less than 7 is acidic
pH more than 7 is basic
how do you do sig figs for concentration
the number of decimal places in pH is equal to the number of sig figs in concentration
how to calculate pH
pH = -log [H+(aq)]
how to calculate concentration
[H+(aq)] = 10^-pH
what are the methods of measuring pH
pH paper- not precise
pH meter- digital reading
computer- pH probe
what are the methods of measuring pH
pH paper- not precise
pH meter- digital reading
computer- pH probe
