Home
Class 11
CHEMISTRY
The equivalent point in a titration of 4...

The equivalent point in a titration of `40.0mL` of a sodium of a weak monoprotic acid occurs when `35.0mL` of a `0.10M NaOH` solutio has been added. The `pH` of the solution is 5.5 after the addition of `20.0mL` of `NaOH` solution. What is the dissociation constant of the acid ?

Promotional Banner

Similar Questions

Explore conceptually related problems

The equivalent point in titration of 40.0 ml of a solution of a weak monoprotic acid occurs when 35.0 of a 0.10 M NaOH solution has been added . The pH of the solution is 5.75 after the addition of 20.0 ml of NaOH solution . What is the dissociation constant of the acid ?

10mL of 2(M) NaOH solution is added to 200mL of 0.5 (M) of NaOH solution. What is the final concentration?

10mL of 2(M) NaOH solution is added to 200mL of 0.5 (M) of NaOH solution. What is the final concentration?

In the titration of a solution of weak acid, HX with NaOH ,the pH is 5.8 after 10 mL of NaOH solution has been added and 6.40 after 20.0mL of the NaOH has been added. What is the ionisation constant of the acid HX ?

A 40 mL solution of weak base, BOH, is titrated with 0.1 N HCl solution. The pH of the solution is found to be 10.04 and 9.14 after the addition of 5 mL and 20 mL of the acid respectively. The dissociation constant of the base will be

10 mL of 2(M) NaOH solution is added to 200 mL of 0.5 (M) of NaOH solution. What is the final concentration of the resultant solution?

In the titration of a solution of a weak acid HX with NaOH , the pH is 5.8 after 10mL of NaOH solution has been added and 6.40 after 20mL of the NaOH has been affed. What is the ionisation constant of the acid HX ?