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pH Dilution Equation:
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The pH dilution equation estimates the pH change when a strong acid or base solution is diluted with water. It provides an approximation of the final pH based on the initial pH and volume ratio.
The calculator uses the pH dilution equation:
Where:
Explanation: The equation accounts for the logarithmic relationship between hydrogen ion concentration and pH, where dilution decreases concentration and thus increases pH for acids (or decreases pH for bases).
Details: Accurate pH estimation during dilution is crucial for laboratory preparations, chemical manufacturing, and understanding how solution concentrations affect acidity/alkalinity levels.
Tips: Enter initial pH value, initial volume and final volume in liters. All values must be valid (volumes > 0, final volume > initial volume).
Q1: When is this equation applicable?
A: This approximation works best for strong acids and bases where complete dissociation occurs. It's less accurate for weak acids/bases or buffered solutions.
Q2: Why does pH change upon dilution?
A: Dilution decreases the concentration of hydrogen ions (for acids) or hydroxide ions (for bases), leading to pH changes toward neutral (pH 7).
Q3: What are the limitations of this equation?
A: The equation assumes ideal behavior and complete dissociation. It may not account for temperature effects, ionic strength, or buffering capacity in real solutions.
Q4: How accurate is this approximation?
A: For strong acids/bases with significant dilution factors, the approximation is reasonably accurate. For precise calculations, full equilibrium calculations may be needed.
Q5: Can this be used for concentrated solutions?
A: The equation works best for dilute solutions. For highly concentrated solutions, activity coefficients and other factors may need to be considered.