Ionic Strength Calculation: How to Account for All Ions in a Solution?

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To calculate the ionic strength of a solution containing acetic acid, NaCl, and NaOH, all ions present in the solution must be considered. This includes both NaCl and NaOH, as each contributes to the overall ionic strength. The ionic strength is crucial for accurately determining the pKa of acetic acid, especially when using the correction method suggested by Sortwell (2001). Therefore, both the sodium ions (from NaCl and NaOH) and the chloride ions from NaCl should be included in the calculation to ensure an accurate assessment of the undissociated acetic acid concentration.
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Hi,

I have a solution containing acetic acid and NaCl. The solution is adjusted to a particular pH value by adding NaOH. For the calculation of the undissociated acetic acid concentration, I use the correction suggested by Sortwell 2001 (J. Food Prot. 63(2): 222-230 (2000)), which says that I have to account for the ionic strength in order to calculate pKa properly.

But my question is: how do I calculate this ionic strength? Do I only take NaCl into account? Or do I also account for the presence of NaOH?

Thanks!
 
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All ions present in the solution, but I have already answered this question somewhere else :wink:
 
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