A 20.0 mL sample of a 0.20 M solution of the weak diprotic acid `H_(2)A` is titrated with 0.250 M NaOH. The concentration of solution at the second equivalent point is:

0.03 M aqueous solution of a weak monobasic acid solution (K_(a)=10^(-12)) is titrated against a 0.01M NaOH solution. What is the [H^(+)] at the end point?

100 ml of 0.2 M CH_3COOH is titrated with 0.2 M NaOH solution. The pH of of the solution at equivalent point will be ( pKa of CH_3COOH=4.76 )

100 ml of 0.2 M CH3COOH is titrated with 0.2 M NaOH solution. The pH of of the solution at equivalent point will be (pKa of CH3COOH=4.76)

During the titration of a weak diprotic acid (H_(2)A) against a strong base (NaOH) , the pH of the solution half-way to the first equivalent point and that at the first equivalent point are given respectively by:

During the titration of a weak diprotic acid (H_(2)A) against a strong base (NaOH) , the pH of the solution half-way to the first equivalent point and that at the first equivalent point are given respectively by:

During the titration of a weak diprotic acid (H_(2)A) against a strong base (NaOH) , the pH of the solution half-way to the first equivalent point and that at the first equivalent point are given respectively by:

A 25.0 mL. sample of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH of the solution at the points where 24.9 and 25.1 mL of NaOH have been added?