Calculate The Ph During The Titration Of 30.00 Ml Of 0.1000

Henderson-Hasselbalch Equation:

\[ pH = pKa + \log\left(\frac{added}{0.1000 \times 0.030 - added}\right) \]

pH:

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1. What is the Henderson-Hasselbalch Equation?

The Henderson-Hasselbalch equation is used to estimate the pH of a buffer solution during titration. It relates the pH, pKa (acid dissociation constant), and the ratio of the concentration of the conjugate base to the concentration of the weak acid.

2. How Does the Calculator Work?

The calculator uses the Henderson-Hasselbalch equation:

\[ pH = pKa + \log\left(\frac{added}{0.1000 \times 0.030 - added}\right) \]

Where:

\( pH \) — Resulting pH value (dimensionless)
\( pKa \) — Acid dissociation constant (dimensionless)
\( added \) — Amount of titrant added (mol)
\( 0.1000 \times 0.030 \) — Initial moles of acid in solution (0.003 mol)

Explanation: The equation calculates the pH during titration of 30.00 mL of 0.1000 M solution based on the amount of titrant added and the pKa of the acid.

3. Importance of pH Calculation in Titration

Details: Accurate pH calculation is crucial for understanding titration curves, determining equivalence points, and analyzing buffer capacity in acid-base reactions.

4. Using the Calculator

Tips: Enter the pKa value and the amount of titrant added in moles. The added amount must be between 0 and 0.003 mol (the initial moles of acid in 30.00 mL of 0.1000 M solution).

5. Frequently Asked Questions (FAQ)

Q1: What is the range of valid input values?
A: pKa can be any real number, but added moles must be between 0 and 0.003 mol.

Q2: Why does the equation become undefined at certain points?
A: The equation becomes undefined when added = 0 or added = total moles (0.003) because the logarithm of 0 or division by 0 is undefined.

Q3: Can this calculator be used for strong acid-strong base titrations?
A: No, the Henderson-Hasselbalch equation is specifically designed for weak acid-strong base or weak base-strong acid titrations.

Q4: What are the limitations of this equation?
A: The equation assumes ideal behavior, constant temperature, and that activity coefficients are approximately 1. It's less accurate far from the pKa and near the equivalence point.

Q5: How does ionic strength affect the calculation?
A: High ionic strength can affect the accuracy as it changes the activity coefficients, which are assumed to be 1 in the standard equation.