DRUG DELIVERY 1 CHAPTER 3 Physical Properties of Solutions - Vocabulary Flashcards (Video Transcript)

Vocabulary flashcards covering key concepts and terms from the lecture notes on physical properties of solutions, concentrations, and isotonicity.

Solution

A chemically and physically homogeneous mixture of two or more substances in which the solute is dissolved in the solvent.

Binary solution

A solution consisting of two components: solute and solvent.

Solute

The component that is dissolved in the solvent.

Solvent

The component in which the solute is dissolved; water is a common solvent.

Ideal solution

A solution with no change in the physical properties of the components other than dilution; follows Raoult’s law.

Raoult’s Law

In an ideal solution, the vapor pressure of each volatile component equals its pure vapor pressure multiplied by its mole fraction.

Mole fraction

The fraction of moles of a component relative to the total moles in the solution.

Real solution

A solution in which mixing changes physical properties; deviations from Raoult’s law occur.

Non-electrolyte

A solute that does not ionize in water and does not conduct electricity; exhibits regular colligative properties.

Strong electrolyte

A solute that completely ionizes in water, conducts current, and shows colligative properties based on the number of ions.

Weak electrolyte

A solute that partially ionizes; conducts weakly; colligative properties depend on degree of ionization.

Colligative properties

Properties that depend on the number of dissolved solute particles (ions or molecules), not their identity.

Vapor pressure lowering

A colligative property where the solvent’s vapor pressure is reduced by the presence of solute.

Boiling point elevation

A colligative property where the boiling point of the solvent increases due to dissolved solute.

Freezing point depression

A colligative property where the freezing point decreases in the presence of dissolved solute.

Osmotic pressure

The pressure required to stop osmosis; a colligative property proportional to solute particle concentration.

Isotonic solution

A solution with the same osmotic pressure as body fluids; isotonicity can be achieved via E-method (0.9% NaCl) or D-method (0.52°C freezing point depression).

0.9% NaCl solution

A standard isotonic reference (0.009 g/mL NaCl) used in E-method isotonic calculations.

Sodium chloride equivalent (E value)

A factor that converts a substance to an equivalent amount of NaCl for isotonicity calculations.

Table 11.1 E-values

A table listing substances with molecular weight, equivalent ions, and E values used in isotonic calculations.

Table 11.2 Freezing point data

A table of freezing-point depressions for various agents used in isotonic calculations.

Isotonic calculation

The process of determining how much NaCl (or other agent) to add to a solution to achieve isotonicity using E-values and tables.

Osmolarity

Total concentration of osmotically active particles per liter; calculable from concentration and degree of ionization.

Molarity

Moles of solute per liter of solution.

Normality

Gram equivalents of solute per liter of solution; equals molarity when solutes have one replaceable hydrogen.

Percent strength

Quantity of solute per 100 parts of solution (percent w/v or similar).

Ratio strength

1/X:1 part solute per total parts (a way to express concentration as a ratio).