solutions Flashcards
solution
homogeneous (1 phase mixture) even distribution of 1+ pure substance mixed together
solvent
present in the larger quantity
- substance that does the dissolving
solutes
present in the lesser quantity
- substance that gets dissolved in the solvent
aqueous solutions
indicates that water is the solvent and that you’re dealing with a solution
miscibility
2 liquids mix in any proportion
- “like dissolves like”
qualitative (empirical) proerties
electrolytic ability
litmus paper
solution colour
flame colour
ELECTROLYTES
ions in solution allow conductivity
NON-ELECTROLYTES
non-conductive molecular solute
acid has
H+
both red
base has
OH-
both blue
SOLUTION COLOUR
some ions have characteristic colour when dissolve in water. Allows for qualitative identification of the ion
what ions are aqueous
all ions are aqueous as ions only exist in water
FLAME TEST
some ions have a characteristic color of flame, when excited by an external heat source
svante arrhenius explaining solutions
dissolving
dissociation
ionization
low solubility
DISSOLVING
polar molecular solutes mix evenly into water by forming new IMF between the solute and solvent
- “like dissolves like”
DISSOCIATION
soluble ionic compounds break apart into individual ions in water.
- crystal lattice breaks
- explains the conductivity of ionic compounds (charged ions)
IONIZATION
a special type of molecular compound with H+ or COOH-, H2O breaks the bond between the H and the rest of the molecule
in ionization, what is the resulting product
an acid is now in water, making acid conductive from its charged ions
LOW SOLUBILITY
non-polar molecular solute
in any phase change or chemical reaction, the following sequence of events must occur
- breaking reactive bonds (endo.)
- forming product bonds (exo.)
when forming a solution with bonds broken
solutes: ionic- cystal lattice must break
molecular- break IMF’s
solvents: IMF’s between water molecules
when forming a solution with bonds forming
IMF’s between water and the solute
what do we feel the net energy change as
we feel it as a change in temperature
exothermic solution formation
solution gets hotter
reactants require less energy needed to break, products more energy released when forming
endothermic solution formation
solution gets colder
reactants require more energy, less energy comes back in products
why does the endothermic solution feel cold
from the lack of heat
solution concentration
always measures the quantity of solute wihtin a specific quantity of solution
solution concentraion formula
quantity of solute/quantity of solution
percent by mass (% m/m)
mass (g) of solute/ mass (g) of solution x 100%
percent by volume (% v/v)
volume (mL) of solute/ mass (g) of solution x 100%
percent mass by volume (% m/v)
mass (g) of solute/ volume (mL) x 100%
parts per million (ppm)
mass (g) of solute/ mass (g) of solution x 100%
or
mass of solute (mg)/ volume of solution (L)
what is the ppm formula for
very low concentrations
amount concentration (c)
amount (mol)/ volume of solution (L)
real life examples of solution concentrations
IV bag
toothpaste
sunscreen
vinegar
mouth wash
alcohol
amount concentration AKA
molar concetration
molarity
why is amount concentration the most useful type of concentration in chem
chemists need to know exact chemical amounts when solutions are used for chemical reactions and analytical techniques
