July 09, 2020, 02:47:03 PM
Forum Rules: Read This Before Posting

Topic: Calculating the pH of a mixture  (Read 376 times)

0 Members and 1 Guest are viewing this topic.

Offline jordaann.t

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Calculating the pH of a mixture
« on: August 06, 2019, 08:41:01 PM »
Hey everyone, not sure how to answer this question ... attached is the question and what I have tried. Thanks.

Offline chenbeier

  • Sr. Member
  • *****
  • Posts: 1050
  • Mole Snacks: +78/-20
  • Gender: Male
Re: Calculating the pH of a mixture
« Reply #1 on: August 07, 2019, 01:54:54 AM »
Acetic acid is a weak acid. You habe to use the Formula for weak acids to  get the concentration. You can calculate the moles of calciumhydroxide and compare how much you have after neutralization. Maybe have to use the Henderson Hasselbalch equation

Offline Enthalpy

  • Chemist
  • Sr. Member
  • *
  • Posts: 3489
  • Mole Snacks: +287/-57
Re: Calculating the pH of a mixture
« Reply #2 on: August 13, 2019, 06:08:58 AM »
Can acetic acid reach a pH of 1.30 at all? I didn't grasp it properly I guess.

Pure acetic acid weighs 1049g/L and 60.05g/mol, that is, 1L contains 17.5mol.

At 1M the dissociation is only 0.4% and this decreases at higher concentration. So even with little water (which would introduce other limits), 1L and 17.5mol would contain less than 0.07mol H+. This gives a pH less strong than 1.16. I suppose the lesser dissociation doesn't let reach 1.30.

From measured pH=2.4 at 1M, pH=1.3 would need over 10× more concentrated H+ and then the ionization of the acid would be over 10× less, rather 0.04% than 0.4%, putting pH=1.3 out of reach.

Sponsored Links