Chem unit 5 aqueous solutions

ionic compound distinguishable macroscopic properties

conductive → more solute = higher conductivity

ionic compound description of dissolving process

polar H₂O molecules interacts with ions and break the ionic bond, ions separated and randomly distributed throughout the solution, ion-dipole interactions between ions and H₂O molecules

Polar covalent compounds distinguishable macroscopic properties

very low to no conductivity

Polar covalent compounds description of dissolving process

polar H₂O molecules break IMF’s between covalent compounds but not covalent bonds within the molecule, solute molecules randomly distributed, interacting via IMFs with the H₂O constant

Acids distinguishable macroscopic properties

Acidic, pH < 7

Acids description of dissolving process

Acids release an H⁺ ion, H⁺ ion bonds with H₃O ion in solution. Remaining part of acid became an anion (A^-). H₃O and A^- are randomly distributed in solution. Interact via ion-dipole interactions

Bases distinguishable macroscopic properties

basic, pH >7 → (^-OH increase) (pH increase) (H₃O decrease)

Bases description of dissolving process

bases take an H⁺ ion from H₂O molecules, ^-OH less randomly distributed, ion-dipole interactions

Dilution formula

(original molarity) (original vol. in L) = (final molarity)(final vol. in L)