[rentj]

25 mL of 0.1 M CH₃COOH and 25 mL of 0.1 M NaOH are titrated and I want to find the pH of the solution after the neutralization reaction takes place. I read a textbook and it shows the working process as attached.

Can we safely assume that after the neutralization reaction occurs, all the species are in chemical equilibrium? Thus, the remaining 1.5 x 10^-3 mol of CH₃COOH would not readjust its equilibrium in respect to H⁺ and CH₃COO^-? Is it safe to assume so?

Thank you.

[Borek]

Can we safely assume that after the neutralization reaction occurs, all the species are in chemical equilibrium? Thus, the remaining 1.5 x 10^-3 mol of CH₃COOH would not readjust its equilibrium in respect to H⁺ and CH₃COO^-? Is it safe to assume so?

Safe? Yes. True? Almost.

Compare: https://www.chembuddy.com/buffers-with-ICE-table

As you can see from the calculations there is a slight shift of the equilibrium, but it is in most cases negligible.

[mjc123]

Do you mean "10 mL of 0.1M NaOH"? Otherwise the calculation is all wrong.