1. What is Dissociation Constant of Weak Electrolyte?

Definition: The dissociation constant (K_a) is a quantitative measure of the strength of a weak acid or base in solution.

Purpose: It helps chemists understand the extent to which a weak electrolyte dissociates into ions in solution.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( K_a \) — Dissociation constant
• \( C \) — Ionic concentration (mol/L)
• \( \alpha \) — Degree of dissociation (0 to 1)

Explanation: The dissociation constant is calculated by multiplying the ionic concentration by the square of the degree of dissociation.

3. Importance of Dissociation Constant

Details: K_a values help predict acid strength, buffer capacity, and pH of solutions. Lower K_a values indicate weaker acids.

4. Using the Calculator

Tips: Enter the ionic concentration in mol/L and degree of dissociation (between 0 and 1). The degree represents the fraction of molecules that dissociate.

5. Frequently Asked Questions (FAQ)

Q1: What is the range for degree of dissociation?
A: The degree of dissociation (α) ranges from 0 (no dissociation) to 1 (complete dissociation).

Q2: What are typical K_a values for weak acids?
A: Weak acids typically have K_a values between 10^-2 and 10^-12.

Q3: How does concentration affect K_a?
A: K_a is a constant for a given acid at a specific temperature, but this calculator shows how apparent dissociation changes with concentration.

Q4: Can I use this for weak bases?
A: This calculator is designed for weak acids. For weak bases, you would use K_b instead.

Q5: What's the relationship between K_a and pK_a?
A: pK_a = -log₁₀(K_a). Lower pK_a values indicate stronger acids.