u3: solubility Flashcards
are solution compositions fixed or variable?
variable
aqueous solution
where water is the solvent
miscible/immiscible substances
Miscible substances readily combine with each other.
Immiscible substances do not dissolve with each other.
what factors determine solubility?
strength of IMFs and speed of molecules
Molecule Size – the smaller it is, the easier it dissolves
Temperature – increases dissolving ability of solids, most liquids, but decreases solubility of gases
Pressure – does not affect dissolving ability of solids and liquids, but increases solubility of gases
explain “like dissolves like.”
- solute only dissolves in solvent when the attraction between them is stronger than the attraction within themselves.
- Ionic and Polar covalent compounds dissolve in polar solvents.
- Non-polar compounds dissolve in non-polar solvents.
energy in solubility?
needs energy: - forces between particles of solvent must be broken, some imfs in liquid must be broken
gives energy: attraction between liquid and solid
temperature and solubility
- increases solubility in liquid
- decreases in gas: bc. when moving fast, can leave the surface
- all solubilities are temperature dependent; must report temperatures with solubilities.
concentration
- amount of solute present in a specific amount of solution
- concentrated: ratio is large
- dilute: ratio is low
wht concentration do very dilute solutions have?
less than 1%
molarity/molar concentration
mols/L
Arrhenius theory of acids/bases
when acids and bases dissolve in water, they dissociate into their ions
acids disassociate
- dissociates (ionizes) in water to produce one or more hydrogen ions, H+
- gives proton, donor
bases disassociate
dissociates in water to form one or more hydroxide ions, OH-
- takes proton, receiver
limitations of arrhenius theory
- H+ does not exist on its own in solution, it becomes hydrated and turns into H3O+ (hydronium ion)
- not all bases contain hydroxide ions (NH3, alkali metal oxides)
