Final answer:
The given statement is true because osmolarity depends on solute properties, specifically the total number of solute particles. Electrolytes affecting osmolarity more per mass than non-dissociating compounds demonstrate this dependency. This concept is essential in understanding colligative properties, tonicity, and osmotic pressure in solutions.
Step-by-step explanation:
The question concerning whether osmolarity depends upon solute properties can be answered as True. Osmolarity is a colligative property which means that it is influenced by the number of solute particles in a solution rather than their size or other specific properties. When a solute dissociates, such as an electrolyte in water, it increases the number of solute particles, thus affecting the osmolarity. For example, electrolytes dissociate into ions and raise the osmolarity more per mass than non-dissociating compounds like glucose. This directly impacts phenomena such as osmotic pressure and helps maintain the tonicity in biological systems, which is of great importance for cell volume and function.
Furthermore, osmolarity directly relates to tonicity which describes how an extracellular solution can alter cellular volume through osmosis. This osmotic effect is particularly notable when solutions with different osmolarities are separated by a water-permeable membrane that does not allow solute movement. It is important to understand that while the osmotic pressure is directly proportional to the number of solute particles, it is the total concentration of these particles that significantly contributes to colligative properties, such as freezing point depression, boiling point elevation, and vapor pressure.
Therefore, the measurement of colligative properties like osmotic pressure allows for the determination of other properties such as the solute's molar mass, and demonstrates how osmolarity is inherently linked to the nature and concentration of solute particles in a solution.