Chemistry Forums for Students > Undergraduate General Chemistry Forum

Weak Acid-Strong Base Neutralization

(1/1)

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:

--- Quote from: rentj on March 06, 2024, 10:04:30 AM ---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?
--- End quote ---

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.

Navigation

[0] Message Index