Why in a strong acid and strong bases reaction, a drop of acid added would not change its PH dramatically but has a big drop near the equivalent point?

PH scal is a logarithmic scale which means PH 3 is10 times more concentrated in hydrogen ions then PH4. PH scale is therefore the negative of hydrogen concentration. Now When a drop of atrong acid, even if the drop has a high concentration of hydrogen ions, the concentration in the total solution is insignificant, hence the PH does not increase much. Nevertheless, near the equavalent point where most of the strong base had been neutralised by the strong acid which leaves a fairly neutralised solution at around PH 6. in this case, even a little drop of the strong acid can change the PH dramatically because the concentration of hydrogen ions in the acid has a direct impact on the excess hydrogen ion concentration of the solution without the buffering effect from the neutralising reaction.

GX
Answered by Grace X. Chemistry tutor

4085 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

What is the charge of iron in the following complex: [Fe(H2O)6]Cl2 ?


What is hybridisation?


What is the structure of fluoroform (CFH3)? Does it have a dipole, explain your answer.


How is the bonding in NH3 and what does this entail for its electron-domain geometry and molecular geometry?


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences