A weak acid `(HA)` is titrated with `N//100 NaOH`. What will be the `pH` when `50%` of titration is completed. Given `K_(a)=1^(-4)` & concentration of `HA=0.1M`

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

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)]

A 0.1 M solution of a weak acid HA is titrated by NaOH slowly. The titration curve observed is given. ka = 4 xx 10^(-5) at 25^(@) C. The correct observation for the curve will be:

0.1 M acetic acid solution is titrated against 0.1M NaOH solution. What would be the difference in pH between 1/4 and 3/4 stages of neutralisation of acid ?

0.1 M acetic acid solution is titrated against 0.1M NaOH solution. What would be the difference in pH between 1/4 and 3/4 stages of neutralisation of acid ?