Diluting Aqueous Solution of Weak Electrolyte by 100 times

When an aqueous solution of a weak electrolyte is diluted by 100 times, several changes occur in the solution. Let's explore the details of this process.

1. Introduction to Weak Electrolytes
- A weak electrolyte is a substance that partially dissociates into ions when dissolved in water.
- Unlike strong electrolytes, which completely ionize, weak electrolytes only dissociate to a limited extent.
- Examples of weak electrolytes include weak acids (e.g., acetic acid) and weak bases (e.g., ammonia).

2. Understanding Dilution
- Dilution refers to the process of reducing the concentration of a solute in a solution by adding more solvent.
- In this case, we are diluting an aqueous solution of a weak electrolyte by 100 times.
- Dilution increases the volume of the solution while keeping the amount of solute constant.

3. Changes in Concentration and Volume
- When the aqueous solution of a weak electrolyte is diluted by 100 times, the concentration of the weak electrolyte decreases by a factor of 100.
- For example, if the initial concentration of the weak electrolyte is 0.1 M, it will become 0.001 M after dilution.
- The volume of the solution increases by a factor of 100 due to the addition of more solvent.

4. Effect on Ionization and Dissociation
- Dilution affects the extent of ionization and dissociation of weak electrolytes.
- Since weak electrolytes only partially dissociate into ions, dilution increases the ratio of solvent molecules to solute molecules.
- This decrease in solute concentration shifts the equilibrium towards the undissociated form of the weak electrolyte.

5. Effect on Conductivity
- Dilution of a weak electrolyte decreases its conductivity.
- Conductivity is a measure of the ability of a solution to carry an electric current, which is directly related to the concentration of ions in the solution.
- As the concentration of the weak electrolyte decreases, the number of ions available to carry the current also decreases, resulting in lower conductivity.

6. pH Changes
- Dilution can affect the pH of a solution containing a weak electrolyte, especially weak acids and bases.
- For example, when a weak acid is diluted, the concentration of H+ ions decreases, resulting in a higher pH (i.e., a more basic solution).
- Conversely, dilution of a weak base leads to a decrease in OH- ions concentration, resulting in a lower pH (i.e., a more acidic solution).

In conclusion, when an aqueous solution of a weak electrolyte is diluted by 100 times, the concentration of the weak electrolyte decreases by a factor of 100, the volume of the solution increases, and the extent of ionization and dissociation decreases. This results in lower conductivity and potential changes in pH, depending on the nature of the weak electrolyte.