100 ml 0.1 M H_3PO_4 solution is being titrated with 0.1 M NaOHsolution. The pH of the reaction mixture keeps increasing with addition of NaOH. The successive dissociation constant of H_3PO_4 " are "10^(-3) , 10 ^(-6) and 10^(-14)respectively.What is the pH of the solution after adding 150 ml of NaOH solution?

100 ml 0.1 M H_3PO_4 solution is being titrated with 0.1 M NaOHsolutio

1.	100 ml 0.1 M H_3PO_4 solution is being titrated with 0.1 M NaOHsolution. The pH of the reaction mixture keeps increasing with addition of NaOH. The successive dissociation constant of H_3PO_4 " are "10^(-3) , 10 ^(-6) and 10^(-14)respectively.What is the pH of the solution after adding 150 ml of NaOH solution?
Answer» <html><body><p>`<a href="https://interviewquestions.tuteehub.com/tag/3-301577" style="font-weight:bold;" target="_blank" title="Click to know more about 3">3</a>`<br/>`6`<br/>`6. <a href="https://interviewquestions.tuteehub.com/tag/7-332378" style="font-weight:bold;" target="_blank" title="Click to know more about 7">7</a>` <br/>`5.3`</p><a href="https://interviewquestions.tuteehub.com/tag/solution-25781" style="font-weight:bold;" target="_blank" title="Click to know more about SOLUTION">SOLUTION</a> :`<a href="https://interviewquestions.tuteehub.com/tag/ph-1145128" style="font-weight:bold;" target="_blank" title="Click to know more about PH">PH</a> = P^(Ka_2)= 6`</body></html>