1. What is pH at Equivalence Point?

The equivalence point in a titration is the point at which the amount of titrant added is stoichiometrically equivalent to the amount of analyte present. The pH at this point depends on the nature of the acid and base being titrated.

2. How Does the Calculator Work?

The calculator determines pH based on the titration type:

Where:

• Strong Acid-Strong Base: pH = 7.0 at equivalence point
• Weak Acid-Strong Base: pH > 7.0 at equivalence point
• Strong Acid-Weak Base: pH < 7.0 at equivalence point
• Weak Acid-Weak Base: pH ≈ 7.0 at equivalence point

Explanation: The pH at equivalence point depends on the salt formed during titration and its hydrolysis behavior.

3. Importance of pH Calculation in Titration

Details: Determining the pH at equivalence point is crucial for selecting appropriate indicators and understanding the titration curve behavior in acid-base titrations.

4. Using the Calculator

Tips: Enter the volume titrated (typically 25 mL in this case), select the acid and base types, and provide the concentration. The calculator will estimate the pH at the equivalence point.

5. Frequently Asked Questions (FAQ)

Q1: Why is pH 7 for strong acid-strong base titration?
A: The salt formed (e.g., NaCl) doesn't hydrolyze, resulting in a neutral solution with pH = 7.

Q2: Why is pH > 7 for weak acid-strong base titration?
A: The conjugate base of the weak acid hydrolyzes water, producing OH⁻ ions and making the solution basic.

Q3: Does volume affect the pH at equivalence point?
A: No, the pH at equivalence point depends only on the nature of the acid and base, not on their concentrations or volumes.

Q4: What factors determine the exact pH value?
A: For weak acid/base titrations, the exact pH depends on the dissociation constant (Ka or Kb) of the weak electrolyte.

Q5: How accurate is this calculator?
A: This provides an estimation. For precise calculations, specific Ka/Kb values would be needed for weak acid/base titrations.