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Jun 29
Dilution law refers to a principle in chemistry that states that the concentration of a solute in a solution is inversely proportional to the volume of the solvent it is dissolved in. This means that as more solvent is added to a solution, the concentration of the solute decreases. The dilution law is often expressed as the equation C1V1 = C2V2, where C1 and V1 are the initial concentration and volume of the solution, and C2 and V2 are the final concentration and volume of the solution after dilution.
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Google Gemini AI
Jun 29
Dilution Law (Ostwald's Dilution Law)
The dilution law, also known as Ostwald's dilution law, is an empirical equation that describes the decrease in the dissociation of a weak electrolyte as its solution is diluted.
Formula:
```
K_a = K_ax^2
```
Where:
- K_a is the ionization constant of the weak electrolyte in the diluted solution
- K_ax is the ionization constant of the weak electrolyte in the concentrated solution
- x is the dilution factor, which is equal to the volume of the diluted solution divided by the volume of the concentrated solution
Explanation:
When a weak electrolyte is diluted, the concentration of its ions decreases. As a result, the equilibrium shifts towards the formation of the undissociated electrolyte, reducing the degree of dissociation. The ionization constant K_a decreases with increasing dilution, as the fraction of ions in the solution decreases.
The dilution law allows us to calculate the ionization constant of a weak electrolyte in a diluted solution, given its ionization constant in a concentrated solution and the dilution factor.
The dilution law, also known as Ostwald's dilution law, is an empirical equation that describes the decrease in the dissociation of a weak electrolyte as its solution is diluted.
Formula:
```
K_a = K_ax^2
```
Where:
- K_a is the ionization constant of the weak electrolyte in the diluted solution
- K_ax is the ionization constant of the weak electrolyte in the concentrated solution
- x is the dilution factor, which is equal to the volume of the diluted solution divided by the volume of the concentrated solution
Explanation:
When a weak electrolyte is diluted, the concentration of its ions decreases. As a result, the equilibrium shifts towards the formation of the undissociated electrolyte, reducing the degree of dissociation. The ionization constant K_a decreases with increasing dilution, as the fraction of ions in the solution decreases.
The dilution law allows us to calculate the ionization constant of a weak electrolyte in a diluted solution, given its ionization constant in a concentrated solution and the dilution factor.
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