1. What is Degree of Dissociation?

Definition: The Degree of Dissociation is the extent of generating current carrying free ions, which are dissociated from the fraction of solute at a given concentration.

Purpose: It helps quantify how much a weak electrolyte dissociates into ions in solution.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( \alpha \) — Degree of Dissociation
• \( K_a \) — Dissociation Constant of Weak Acid
• \( C \) — Ionic Concentration (mol/L)

Explanation: The degree of dissociation is calculated as the square root of the ratio of the acid dissociation constant to the ionic concentration.

3. Importance of Degree of Dissociation Calculation

Details: Understanding the degree of dissociation is crucial for predicting the behavior of weak electrolytes in solution, including their conductivity and pH.

4. Using the Calculator

Tips: Enter the dissociation constant (Ka) of the weak acid and the ionic concentration (in mol/L). All values must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What is the range for degree of dissociation?
A: For weak electrolytes, α typically ranges between 0 and 1, where 0 means no dissociation and 1 means complete dissociation.

Q2: How does concentration affect degree of dissociation?
A: For weak electrolytes, the degree of dissociation increases with dilution (lower concentration).

Q3: What's a typical Ka value for weak acids?
A: Weak acids typically have Ka values between 10^-2 and 10^-10. For example, acetic acid has Ka ≈ 1.8 × 10^-5.

Q4: Can this formula be used for strong electrolytes?
A: No, this formula is only valid for weak electrolytes. Strong electrolytes are considered completely dissociated (α ≈ 1).

Q5: What are the limitations of this calculation?
A: This is an approximation that becomes less accurate for higher concentrations or very weak electrolytes where other factors become significant.