When substances are mixed, mass is conserved, but volume might not be because particles fill gaps between each other.
"Like dissolves like." Whether a solute can dissolve in a solvent depends on a balance of attractive forces (solute-solvent vs. solvent-solvent and solute-solute). This means that polar substances tend to dissolve in other polar substances, and non-polar substances tend to dissolve in non-polar substances.
When molecular (covalent) substances dissolve, their particles remain intact but separate from each other.
When ionic solids dissolve, their ionic bonds are actually broken, producing free-floating ions. This is called dissociation.
The concentration of a solution is measured in molarity, meaning mol/L.
The greater the concentration of ions dissolved in water, the greater the electrical conductivity of the solution.
Based on polarity or ionic charge, predict whether a covalent or ionic species will dissolve in a given solvent.
Determine the concentration of a solution.
Perform dilution and mixing calculations.
Describe the effect of a solvent on electrical conductivity.
Perform stoichiometric calculations involving solutions.