when the Ka value changes, the pH value also changes.
We must keep in mind that every chemical reaction has an equilibrium constant K, and that K fluctuates as the temperature changes, in order to answer this problem.
If an exothermic reaction occurs,:
K value drops as temperature rises.
K value rises as temperature drops If the reaction is endothermic, the temperature rises and the K value rises.
K value drops as temperature rises
Since the Henderson-Hasselbalch equation includes the Ka value when there is a buffer, we know that when the Ka value changes, the pH value also changes:
[tex]PH= PKa+log \frac{A}{HA}[/tex]
Small additions of acid or base can be neutralized by it, keeping the pH of the solution largely constant. For procedures and/or reactions that call for particular and stable pH ranges, this is significant.
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