If you double the concentration of a non diffusible solute – If you double the concentration of a non-diffusible solute, you will witness a cascade of profound effects on osmotic pressure, diffusion, and equilibrium. This alteration has far-reaching implications for colligative properties, membrane potential, and the physiological functioning of biological systems.
As we delve into this topic, we will unravel the intricate relationship between solute concentration and these fundamental processes, exploring the underlying mechanisms and their significance in various biological contexts.
Osmotic Pressure: If You Double The Concentration Of A Non Diffusible Solute
Doubling the concentration of a non-diffusible solute increases the osmotic pressure by a factor of 2. Osmotic pressure is the minimum pressure required to prevent the flow of water across a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration.
The osmotic pressure of a solution is directly proportional to the concentration of the solute, as expressed by the following equation:
π = MRT
Where:
- π is the osmotic pressure
- M is the molar concentration of the solute
- R is the ideal gas constant (0.0821 Latm/(molK))
- T is the absolute temperature (in Kelvin)
Diffusion and Equilibrium
Doubling the concentration of a non-diffusible solute decreases the rate of diffusion by a factor of 2. Diffusion is the movement of molecules from an area of high concentration to an area of low concentration. The rate of diffusion is proportional to the concentration gradient, which is the difference in concentration between the two areas.
When a non-diffusible solute is present, it creates a concentration gradient that opposes the diffusion of other molecules. This is because the non-diffusible solute cannot move across the membrane, so it effectively blocks the movement of other molecules.
Equilibrium is not reached when a non-diffusible solute is present because the concentration gradient is constantly being maintained. In a system with a non-diffusible solute, the concentration of the solute will be higher on one side of the membrane than the other.
This concentration gradient will drive the diffusion of other molecules from the side with the lower concentration to the side with the higher concentration. However, the non-diffusible solute will prevent the molecules from reaching equilibrium, as it will block their movement across the membrane.
Colligative Properties
Doubling the concentration of a non-diffusible solute affects colligative properties such as boiling point elevation and freezing point depression. Colligative properties are properties that depend on the concentration of a solute in a solution, but not on the nature of the solute.
Boiling point elevation is the increase in the boiling point of a solution compared to the boiling point of the pure solvent. Freezing point depression is the decrease in the freezing point of a solution compared to the freezing point of the pure solvent.
Doubling the concentration of a non-diffusible solute will double the boiling point elevation and double the freezing point depression. This is because the colligative properties are directly proportional to the concentration of the solute. For example, if the boiling point of pure water is 100°C, then the boiling point of a solution with a non-diffusible solute at a concentration of 1 mol/L will be 100.51°C.
If the concentration of the solute is doubled to 2 mol/L, then the boiling point will be 101.02°C.
Membrane Potential
Doubling the concentration of a non-diffusible solute on one side of a membrane affects the membrane potential. Membrane potential is the difference in electrical potential between the inside and outside of a cell. It is created by the movement of ions across the membrane.
When a non-diffusible solute is present on one side of the membrane, it creates a concentration gradient for ions. This concentration gradient drives the movement of ions across the membrane, which creates a membrane potential.
The Nernst equation is used to calculate the membrane potential. The Nernst equation is:
E = (RT/zF)ln([Ion] out/[Ion] in)
Where:
- E is the membrane potential
- R is the ideal gas constant (8.314 J/molK)
- T is the absolute temperature (in Kelvin)
- z is the valence of the ion
- F is the Faraday constant (96,485 C/mol)
- [Ion] outis the concentration of the ion outside the cell
- [Ion] inis the concentration of the ion inside the cell
Doubling the concentration of a non-diffusible solute on one side of the membrane will change the concentration gradient for ions. This will change the membrane potential. For example, if the concentration of a non-diffusible solute is doubled on the outside of a cell, then the membrane potential will become more negative.
Biological Implications
Doubling the concentration of a non-diffusible solute in biological systems can have a number of physiological implications. For example, if the concentration of a non-diffusible solute is doubled in the extracellular fluid, then the cells will lose water by osmosis.
This can lead to dehydration and a number of other health problems. Conversely, if the concentration of a non-diffusible solute is doubled in the intracellular fluid, then the cells will gain water by osmosis. This can lead to cell swelling and a number of other health problems.
The concentration of non-diffusible solutes is also important for the function of many proteins. For example, the activity of some enzymes is affected by the concentration of ions in the surrounding environment. If the concentration of a non-diffusible solute is doubled, then the concentration of ions in the surrounding environment will change.
This can affect the activity of enzymes and lead to a number of physiological changes.
FAQ
What happens to osmotic pressure when the concentration of a non-diffusible solute is doubled?
Doubling the concentration of a non-diffusible solute doubles the osmotic pressure.
How does doubling the concentration of a non-diffusible solute affect the rate of diffusion?
Doubling the concentration of a non-diffusible solute does not affect the rate of diffusion.
Why is equilibrium not reached when a non-diffusible solute is present?
Equilibrium is not reached when a non-diffusible solute is present because the non-diffusible solute cannot cross the semipermeable membrane, creating an imbalance in solute concentration across the membrane.
