Essay on Chemistry : A Non Electrolyte Compound
Colligative properties are properties of a solution that depend on the amount of solute dissolved, and not dependent on the identity of the solute. The colligative properties studied in this current chapter of chemistry are: vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
The van’t Hoff factor for a solute is equivalent to the number of particles, in moles, will break apart in the solvent. When an electrolyte is dissolved in water, the compound separates into ions. The number of moles of the total ions resulted after dissolution is the van’t Hoff factor for that particular solute.
The dissociation equation is a chemical equation that demonstrates the separation of an ionic compound when in a solution. The chemical formula of the ionic compound is broken into its ions. An example of a dissolution equation is: Na〖Cl〗_((s)) □(→┴(H_2 O) ) Na^+(aq)+〖Cl〗^-(aq). The van’t Hoff factor for this solution is two. When one mole of sodium chloride is dissolved in water, the ionic compound is broken into one mole of sodium ions and one mole of chloride ions, which is a total of two moles of solute.
The ionization equation is a chemical…