Unit test 4- Solutions Flashcards
what is water
the universal solevant
homogenous mixture
2 distinct layers
solute
a substance that is lesser in quantity
solevant
a substance in the greater quantity
solution
a homogenous mixture of 2 or more substances (appear uniform)
aqueous solution
transparent and contains water
electrolyte
-a compound that dissolves in water producing a solution that conducts electricity
-a salt solution
miscible
2 substances mix to be heterogenous
immiscible
2 substances cannot mix together, form 2 seperate layers
surfactant
-lower liquid surface tension
-have both hydrophobic & hydrophilic parts
-hydrophobic
-hydrophilic
hydrophobic: interacts with dirt & oil
hydrophilic: interact with water
where is ppm used
-enviro. chemistry
ex: Reporting effects of toxic substances
what is the effects of heat on solubility of solids vs. gases
solids- greater solubility at higher temps
gases- lower solubility at higher temps
properties of acids
-start with H
-conduct electricity
-taste sour
-are corrosive
-react with metals to produce H2
*PH below 7
-litmus paper red
how does crystallization happen
rapid evaporation forms small crystals, slow evaporation forms large crystals
properties of Bases
-have hydroxide or carbonate in formula (produce OH- in water)
-taste bitter, feel slippery
-conduct electricity in solution
-PH above 7
-turn litmus paper blue
acids
molecular compounds that ionization in H2O to form hydrogen ions H+
ionization
formation of ions from an uncharged molecule
bases
ionic hydroxide compounds that dissociate in H2O to produce OH-
flaws to Arrhenius theory
-how Na2CO3 or NH3 can act like acids
-H+ ions don’t actually exist in water
revisions to Arrhenius theory- acids
H+ ions react with H2O to produce H3O (hydronium ions)
–> strong acids react completely with water
–> weak acids react somewhat with water
revisions to to Arrhenius theory- bases
–> strong bases dissociate in 100% in H2O producing OH- ions
–> weak bases produce less OH- ions
what is Ph
-is a way of calculating the hydrogen ion concentration of a solution
-power of hydrogen
what is pH measured in
logarithmic scale
