How will the osmotic pressure of an aqueous solution change as evaporation occurs?
does it even change? or does it increase?
evaporation will increase concentration, correct?
Evaporation of an aqueous solution can indeed impact the osmotic pressure of the solution. As water evaporates, the solutes in the solution become more concentrated, leading to an increase in osmotic pressure.
To understand this process, let's first explain what osmotic pressure is. Osmotic pressure is the pressure required to prevent the net flow of solvent molecules across a semipermeable membrane, caused by the concentration gradient of solute particles.
During evaporation, only the solvent (water) molecules evaporate, while the solute particles remain in the solution. As water evaporates, the volume of the solution decreases, resulting in a higher concentration of solute particles. This increase in concentration leads to a higher osmotic pressure.
To calculate the exact change in osmotic pressure caused by evaporation, you would need to know the initial concentration of the solute and the extent of evaporation. Using this information, you could employ thermodynamic equations, such as the van 't Hoff equation, to determine the change in osmotic pressure.
In summary, as water evaporates from an aqueous solution, the remaining solute particles become more concentrated, leading to an increase in osmotic pressure.