Why does the OH react with HA and not H3O+?

  • Thread starter Thread starter motornoob101
  • Start date Start date
Click For Summary
SUMMARY

In the titration of a weak acid (HA) with a strong base, hydroxide ions (OH-) preferentially react with HA rather than hydronium ions (H3O+) to achieve neutralization. This occurs because hydroxide ions effectively deprotonate HA, leading to the neutralization of remaining HA molecules. The reaction dynamics favor the interaction between OH- and HA over H3O+, as hydroxide can abstract protons from both species but is more effective in neutralizing the weak acid directly.

PREREQUISITES
  • Understanding of acid-base chemistry, particularly weak acids and strong bases.
  • Familiarity with titration techniques and their applications.
  • Knowledge of proton transfer mechanisms in aqueous solutions.
  • Basic grasp of chemical equilibrium concepts.
NEXT STEPS
  • Research the titration process of weak acids with strong bases in detail.
  • Explore the role of hydroxide ions in acid-base reactions.
  • Study the concept of proton abstraction and its implications in chemical reactions.
  • Learn about the equilibrium dynamics of weak acids and their conjugate bases.
USEFUL FOR

Chemistry students, educators, and professionals involved in analytical chemistry or laboratory work focusing on acid-base titrations.

motornoob101
Messages
45
Reaction score
0
In titrating HA, the weak acid with a strong base, why does the OH- ions from the strong base react with the HA atom (and neutralize it) rather than say react with the H3O+ to form complete neutralization? Just curious. Thanks.
 
Physics news on Phys.org
HA donates protons to water regardless of whether the base is present or not however the hydroxide can neutralize the remaining HA molecules. Ultimately hydroxide is going to prefer the latter over the former.
 
motornoob101 said:
In titrating HA, the weak acid with a strong base, why does the OH- ions from the strong base react with the HA atom (and neutralize it) rather than say react with the H3O+ to form complete neutralization? Just curious.
Thanks.

Hydroxide deprotonates weak acids and hydronium ion alike. In a basic solution, hydroxide abstracts acidic protons from both molecules.
 

Similar threads

Chemistry Are there typos in this snippet causing confusion?
  • · Replies 2 ·
Replies
2
Views
2K
Chemistry Why is HCl an Arrhenius acid but hydrogen carbonate isn't?
  • · Replies 4 ·
Replies
4
Views
2K
How does a buffer actually work?
  • · Replies 1 ·
Replies
1
Views
2K
Chemistry Comparing methods of computing pH at equivalence point in titration
  • · Replies 4 ·
Replies
4
Views
2K
Chemistry PH Indicator and Endpoint Observations
  • · Replies 3 ·
Replies
3
Views
2K
Finding acid dissociation rate constant from titration
  • · Replies 1 ·
Replies
1
Views
2K
Can you make pure water acidic by adding free protons to it?
  • · Replies 6 ·
Replies
6
Views
885
Comparing a hydronium with a hydroxide in a weak acid solution (0.1M)
  • · Replies 9 ·
Replies
9
Views
2K
Doubt about calculating the solubility of lamivudine (3TC)
  • · Replies 48 ·
2
Replies
48
Views
9K
Chemistry Understanding how to calculate pH of a buffer solution
  • · Replies 2 ·
Replies
2
Views
2K