10 mL of 0.2 M HA is titrated with 0.2 M NaOH solution. Calculate change in pH between 50% of equivalence point to equivalence point.
`[K_(a)` of HA `=10^(-5)]`

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)

10 mL of 0.1 M tribasic acid H_(3)A is titrated with 0.1 M NaOH solution. What is the ratio of ([H_(3)A])/([A^(3-)]) at 2^(nd) equivalence point ? Given K_(1)=7.5xx10^(-4), K_(2)=10^(-8), K_(3)=10^(-12) .

0.1 M of HA is titrated with 0.1 M NaOH, calculate the pH at end point. Given K_(a)(HA)=5xx10^(-5) and alpha lt lt 1

0.1 M of HA is titrated with 0.1 M NaOH, calculate the pH at end point. Given K_(a)(HA)=5xx10^(-5) and alpha lt lt 1