What is the Best Method for Titration of a Weak Acid with a Strong Base?

  • Thread starter Thread starter [aq]
  • Start date Start date
  • Tags Tags
    Acid Base Weak
Click For Summary

Discussion Overview

The discussion revolves around the titration of a weak acid with a strong base, specifically focusing on determining the initial molarity of an unknown weak acid using a standardized sodium hydroxide solution. Participants explore the implications of the equivalence point's pH and the role of buffers in this context.

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested
  • Homework-related

Main Points Raised

  • One participant questions the pH at the equivalence point when titrating a weak acid with a strong base, suggesting it is greater than 7 but lacking specific information about the acid.
  • Another participant asserts that buffers are not relevant in this context, emphasizing that the final pH at the equivalence point will be determined by the salt formed from the reaction.
  • A participant introduces a related question about the advantages of using a weak base, such as calcium carbonate, to neutralize a strong acid, implying that it may produce less alkaline conditions.
  • There are inquiries about the final pH when adding calcium carbonate to a neutral solution, with some participants questioning the practicality of this approach.
  • One participant expresses a lack of ideas or solutions regarding the titration process, indicating uncertainty in their understanding.

Areas of Agreement / Disagreement

Participants exhibit disagreement regarding the relevance of buffers in the titration process and the implications of using weak versus strong bases for neutralization. The discussion remains unresolved, with multiple viewpoints presented.

Contextual Notes

Participants have not provided specific information about the weak acid, which may limit the discussion's applicability. The relationship between the pH at the equivalence point and the properties of the acid remains unclear.

[aq]
Messages
6
Reaction score
0
Hiya,

Im trying to determine the initial molarity of an unknown acid, sooo I am trying to titrate it with standardized sodium hydroxide solution (0.1M). But I am having a load of problems figuring out what the heck I am supposed to do since i am told the acid is a weak acid.

If I am titrating a weak acid using a strong base the equivalence point is at a pH level greater than 7 correct?

But I am not supplied with information regarding anything about the acid except that it is weak, and nothing about the pH at the equivalence point!

How would i go about doing this titration ? Does buffers have anything to do with this (since according to my textbook, the acid-base buffer should form around the halfway point to the equivalence point).
 
Chemistry news on Phys.org
Buffers do not have anything to do with it since strong acid/bases have no relation to buffers.

here are some hints:

Titrate to completion, at the equivalence point, that is when the acid and base have reacted in stoichiometric equivalence, the final pH will be determined by the salt formed in the reaction.

from this pH you should be able to determine the pKa of the weak acid.
 
Why is it better to use a weak base(such as calcium carbonate) to neutralise strong acid (such as hcl) rather than strong base?

Thank you so much
 
Please don't hijack threads.

And remember we want you to try first. You do have some ideas, don't you?
 
Last edited:
no i don't have a correct answer but i think it is because weaker acid is less likely to make the solution alkali therefore acidic salt is produced
 
If you start with a neutral solution, and you add calcium carbonate, what will be the final pH?
 
Borek said:
If you start with a neutral solution, and you add calcium carbonate, what will be the final pH?

The use of Calcium Carbonate might be a choice to employ the insolubility of calcium carbonate after all of the acid is neutralized, but is this practical/useful?

This "hijack" was also on another board, and I gave a response there.

BETTER: Start a new topic and not continue this "Calcium Carbonate - Strong Acid" topic here.
 

Similar threads

Chemistry Are there typos in this snippet causing confusion?
  • · Replies 2 ·
Replies
2
Views
2K
Concentrations at equilibrium (strong base weak acid)
  • · Replies 2 ·
Replies
2
Views
2K
Comparing a hydronium with a hydroxide in a weak acid solution (0.1M)
  • · Replies 9 ·
Replies
9
Views
2K
Chemistry Book seems to say that we can have weak acid and weak conjugate base
  • · Replies 2 ·
Replies
2
Views
2K
How can I prepare a 0.1M NaOAc buffer at pH 5 using titration?
  • · Replies 4 ·
Replies
4
Views
5K
Equivalence point in acid-base titration
  • · Replies 3 ·
Replies
3
Views
2K
Chemistry Is pH of strong acid strong base titration always 7 at stoichiometric point?
  • · Replies 2 ·
Replies
2
Views
2K
At what temperature does citric acid decay?
  • · Replies 5 ·
Replies
5
Views
5K
Solution of salt of a weak base and salt of a weak acid
  • · Replies 15 ·
Replies
15
Views
8K
Chemistry How to take into account autoprotolysis in weak base solution?
  • · Replies 8 ·
Replies
8
Views
2K