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Titration of Polyprotic Acids with a Strong Base01:23

Titration of Polyprotic Acids with a Strong Base

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Titration of a polyprotic acid, which contains multiple ionizable protons, involves distinct dissociation steps, each with its own dissociation constant (Ka). Each successive Ka is weaker than the previous one. In the titration of a polyprotic acid like sulfurous acid with a strong base such as sodium hydroxide, the base first neutralizes the initial ionizable proton, forming an intermediate species (e.g., hydrogen sulfite ions). This step's titration curve resembles that of a weak...
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Complexation Equilibria: Factors Influencing Stability of Complexes01:09

Complexation Equilibria: Factors Influencing Stability of Complexes

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In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
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Composition of Polyprotic Acid Solutions as a Function of pH01:19

Composition of Polyprotic Acid Solutions as a Function of pH

478
Polyprotic acids of the type H2M constitute two ionizable protons. As a result, on titration with a base, they exhibit two equivalence points in the titration curve. During titration, the species H2M, HM−, and M2− will be present in the solution at different points. The fractions of H2M, HM−, and M2− present at the various instances of the titration are denoted by α0, α1, and α2, respectively.
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Titration of a Polyprotic Acid02:08

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95.6K
A polyprotic acid contains more than one ionizable hydrogen and undergoes a stepwise ionization process.  If the acid dissociation constants of the ionizable protons differ sufficiently from each other, then the titration curve for such polyprotic acid generates a distinct equivalence point for each of its ionizable hydrogens. Therefore, titration of a diprotic acid results in the formation of two equivalence points, whereas the titration of a triprotic acid results in the formation of three...
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Formation of Complex Ions03:45

Formation of Complex Ions

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A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
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Polyprotic Acids03:38

Polyprotic Acids

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Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
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Metastable Shared Proton Complexes in Aqueous Sulfuric Acid Solutions.

Sijia Chen1, Bohak Yoon1, Jiangbo Wu1

  • 1Department of Chemistry, Chicago Center for Theoretical Chemistry, The James Franck Institute, and Institute for Biophysical Dynamics, The University of Chicago, Chicago, Illinois 60637, United States.

The Journal of Physical Chemistry Letters
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Metastable, shared proton contact ion pairs (CIPs) form between anions in sulfuric acid solutions. These ion pairs create stable Zundel-like complexes, revealing new insights into acidic solution behavior.

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Area of Science:

  • Physical Chemistry
  • Solution Chemistry
  • Computational Chemistry

Background:

  • Aqueous sulfuric acid solutions are fundamental in many chemical processes.
  • Understanding ion pairing and solvation is crucial for predicting solution behavior.
  • Previous models often simplify interactions in concentrated acidic media.

Purpose of the Study:

  • To investigate the formation and stability of shared proton contact ion pairs (CIPs) in aqueous sulfuric acid.
  • To elucidate the structural and energetic characteristics of these ion pairs.
  • To explore the role of solvation and specific interactions in stabilizing these complexes.

Main Methods:

  • *Ab initio* molecular dynamics (AIMD) simulations.
  • Free energy sampling techniques.
  • Quantum mechanics (QM) calculations.
  • Radial distribution function (RDF) analysis.

Main Results:

  • Identified the formation of metastable, shared proton contact ion pairs (CIPs) between anions.
  • Characterized the Zundel-like complex structure with strong inter-anion hydrogen bonding.
  • Quantified the free energy profile and dissociation barrier for anion pairing.
  • Revealed the significant contributions of induction interactions and solvation effects.

Conclusions:

  • Shared proton contact ion pairs (CIPs) represent a key structural motif in aqueous sulfuric acid solutions.
  • Induction and solvation effects play a critical role in stabilizing these ion pairs.
  • Aqueous acidic solutions exhibit complex behavior beyond simple hydronium dissociation.