1. What is the Dissociation Constant?

The dissociation constant (Ka) quantifies the strength of an acid in solution. It represents the equilibrium constant for the dissociation reaction of an acid into its conjugate base and a proton. A higher Ka value indicates a stronger acid.

2. How Does the Calculator Work?

The calculator uses the dissociation constant equation:

Where:

• \( [H^+] \) — Hydrogen ion concentration (M)
• \( [A^-] \) — Conjugate base concentration (M)
• \( [HA] \) — Weak acid concentration (M)

Explanation: The equation quantifies the extent to which an acid donates protons in solution, with higher values indicating stronger acids.

3. Importance of Ka Calculation

Details: Calculating Ka is essential for understanding acid strength, predicting reaction outcomes, and designing buffer solutions in chemistry and biochemistry.

4. Using the Calculator

Tips: Enter all concentrations in molarity (M). All values must be positive numbers greater than zero for accurate calculation.

5. Frequently Asked Questions (FAQ)

Q1: What does a high Ka value indicate?
A: A high Ka value indicates a strong acid that dissociates completely in solution.

Q2: How is pKa related to Ka?
A: pKa is the negative logarithm of Ka (pKa = -log10Ka). Lower pKa values correspond to stronger acids.

Q3: What are typical Ka values for common acids?
A: Strong acids have Ka > 1, while weak acids have Ka < 1. For example, acetic acid has Ka ≈ 1.8×10⁻⁵.

Q4: Does temperature affect Ka values?
A: Yes, Ka values are temperature-dependent as dissociation is an equilibrium process influenced by temperature changes.

Q5: Can this calculator be used for polyprotic acids?
A: This calculator is designed for monoprotic acids. Polyprotic acids have multiple dissociation constants (Ka1, Ka2, etc.).