Question

50 ml of 0. 100 m hcl is titrated with 0. 1500 m naoh. the ph at the equivalence point is:_____.

Answer 1

The answer is 7.

The equivalence point of a titration is when moles of titrant added becomes equal to the moles of sample analyte.

Calculate the pH at equivalence point for a strong acid and strong base reaction.

• The given acid is HCl which is a strong acid and the base NaOH is also a strong base.
• Calculate the moles of acid HCl:

Molarity of $HCl$= 0.100 M

Volume of $HCl$ = 50 mL = 0.050 L

$Moles\ of\ HCl\ = Molarity\ of\ HCl$×$Volume\ of\ HCl\ in\ L$

                      $= 0.100\ M$×$0.050\ L = 0.005\ moles$

• At equivalence point, same moles of base are added and thus it results into complete neutralization. Thus, all the hydrogen ions of acid are neutralized by the hydroxide ions of the base forming only water and neutral salt.
• Thus, the pH at the equivalence point becomes 7 (neutral solution).

To learn more about pH at equivalence point visit:

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