For a lab for acid/base titration with a weak acid/strong base. There was a big

Question

For a lab for acid/base titration with a weak acid/strong base. There was a big difference between the measure pH and the calculated pH for at the initial pH when there was no base added (measured: 1.7, calculated:2.4) and also when the strong base was added past the titration point (measured: 10.8, calculated: 11.8). In this lab there was also a strong acid and strong base titration, however the measured and calculated pH values for this titration were close.

The question is "Do your data exhibit any systematic (always high or always low) errors? If so, why do you think that is?"

Is there some reason as to why the calculated pH is more basic than the theoretical pH for both?

Explanation / Answer

In an acid/base titration weak acid/strong base forms a near Buffer solution whose PH Value is constant even when a strong acid or strong base is added!

So the theoretical values and practical values don't match due to the formation of a buffer solution.

When we consider strong acid and strong base titrations there is no buffer solution in the picture so PH Values are close.

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