When one substance dissolves in another the result is a solution of greater disorder.
All cases of solids dissolving in water are NOT endothermic.
All cases of gases dissolving in water are exothermic.
In general, the larger the charge and the smaller the size of an ion, the more easily it can be hydrated.
The more negative the lattice energy for a solid substance, the less likely that it is able to dissolve in a specific solvent.
Strong electrolytes are those that are mostly ionized in dilute aqueous solutions.
A solution that is described as concentrated would have a higher molarity than a dilute solution.
For a given solution, it would probably be easier to measure the freezing point depression than the boiling point elevation.
A solution is an example of a HOMOGENOUS mixture.
When we describe a solution of a little sugar in water, we describe sugar as SOLUTE and water as SOLVENT.
The reverse of the dissolution process is called PRECIPITATION/CRYSTALIZATION.
A solution that contains dissolved solute in equilibrium at a given temperature with excess undissolved solute is said to be SATURATED.
The ease of the dissolution process depends on two factors: the change in ENTROPY and ENERGY
A process in which the substances involved decrease in energy is called EXOTHERMIC.
The three types of interactions that are useful to consider in assessing the change in heat content on dissolution are SOLUTE-SOLUTE IMFS, SOLUTE-SOLVENT IMFS, SOLVENT-SOLVENT IMFS.
The dissolution process is favored by WEAK solute-solute attractions, by WEAK solvent-solvent attractions, and by STRONG solute-solvent attractions.
The close clustering of solvent molecules around a solute particle is generally called SOLVATION; when the solvent is water it is called HYDRATION.
The lowering of the vapor pressure of a solvent due to the presence of dissolved solute is described by RAOULT'S Law, which states in words that the mole fraction of the solvent multiplied by the vapor pressure...