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Buffer pH Equation After Adding Strong Acid:
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The buffer pH equation calculates the new pH of a buffer solution after adding a strong acid. It's based on the Henderson-Hasselbalch equation and accounts for the consumption of base and formation of conjugate acid when strong acid is added to the buffer system.
The calculator uses the buffer pH equation:
Where:
Explanation: The equation calculates the new pH based on the changed ratio of base to acid concentrations after the strong acid reacts with the buffer components.
Details: Accurate pH calculation is crucial for understanding buffer capacity, predicting pH changes in chemical and biological systems, and designing effective buffer solutions for various applications.
Tips: Enter pKa value, initial base and acid concentrations in mol, and amount of strong acid added in mol. All concentration values must be positive, and added acid should not exceed the available base.
Q1: What happens if too much strong acid is added?
A: If added acid exceeds the initial base concentration, the buffer capacity is exceeded, and the pH will drop significantly according to the strong acid concentration.
Q2: Can this equation be used for weak acid additions?
A: No, this equation is specifically for strong acid additions. Weak acids require different calculations as they partially dissociate.
Q3: What are typical pKa values for common buffers?
A: Common buffers have pKa values around physiological pH (7.4), such as phosphate (pKa 7.2), Tris (pKa 8.1), and acetate (pKa 4.76).
Q4: How does temperature affect the calculation?
A: Temperature affects pKa values. The calculation assumes constant temperature, so pKa should be appropriate for the experimental conditions.
Q5: What if the added amount equals the base concentration?
A: When added acid equals the base concentration, the ratio becomes zero and the logarithm is undefined, indicating complete consumption of the buffer base.