The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.440 moles of a monoprotic weak acid ( K a = 8.3 × 10 − 5 ) is titrated with NaOH , what is the pH of the solution at the half‑equivalence point?

Answer : The pH of solution at the half‑equivalence point is, 4.1

Explanation :

As we known that the titration takes place between strong base and weak acid.

So, at half‑equivalence point of a titration the pH of the solution is equal to the of weak acid.

As we are given:

Now we have to calculate the value of .

The expression used for the calculation of is,

Now put the value of in this expression, we get:

Thus,

Therefore, the pH of solution at the half‑equivalence point is, 4.1

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error