Chem Finals

• Solutions can also be expressed in molality and molarity.
• Molality of a solution is the number of moles of solute per kilogram of solvent.
• Molarity of a solution is the number of moles of solute per liter of solution.
• Moral (m) is the unit of molality
• molar (M) is the unit of molarity
• Solubility is the maximum amount of solute that can dissolve in a solvent at a specific temperature.
• Henry’s law is named after the British Chemist William Henry (1775-1836)
• Colligative properties are influenced by the extent of dissociation of the solute in a solution/ changes in a solution that depend on how much solute (like salt or sugar) is dissolved in it, rather than on the type of solute. Changes like vapor pressure lowering, freezing point depression, boiling point, and osmotic pressure.
• Solutions that depend on the nature of their components can be classified as electrolytic or nonelectrolytic.
• Electrolytes are substances that, when dissolved in water or ionized in a solution, the ions conduct electricity.
• Nonelectrolytic are those that do not ionize in a solution and thus do not conduct electricity.
• Depending on what the solvent is, one mole of any nonelectrolyte will lower the freezing point of a given amount of solvent by a constant amount referred to as the freezing point depression constant (Kf) or the cryoscopic constant.
• Osmosis is a process through which a solvent flows through a semipermeable membrane from less concentrated solution to more concentrated one.
• Semipermeable membrane is a selectively porous material, that only allows certain substances to pass through it.
• Osmotic pressure is the amount of pressure required to stop osmosis.
• Isotonic is when two solutions have the same osmotic pressure.
• Hypotonic is when there is an imbalance between solute concentration with water moving into the cell.
• Hypertonic is when there is an imbalance between solute concentration with water moving out of the cell.