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Related Concept Videos

Titration in Nonaqueous Solvents01:16

Titration in Nonaqueous Solvents

Most acid-base titrations are performed in an aqueous medium. In aqueous titrations, water competes with weaker acids or bases for proton donation or acceptance, leading to ambiguous endpoints in the titration curve. Water also affects the partial ionization of weak acids or bases. For example, water accepts a proton from acetic acid to form hydronium and acetate ions. The hydronium ion formed is a stronger acid than acetic acid, and the acetate ion is a stronger base than water. As a result,...
Leveling Effect and Non-Aqueous Acid-Base Solutions02:11

Leveling Effect and Non-Aqueous Acid-Base Solutions

This lesson defines the leveling effect in acidic and basic solutions and its role in aqueous and non-aqueous solutions. It is essential to understand the competing nature of various species in a chemical system.
The Leveling Effect of a Solvent
A generic acid (HA) reacts with the generic base (B-) to yield the corresponding conjugate base (A-) and conjugate acid (HB):
Titration of Polyprotic Acids with a Strong Base01:23

Titration of Polyprotic Acids with a Strong Base

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 monoprotic...
Titration of Polyprotic Base with a Strong Acid01:18

Titration of Polyprotic Base with a Strong Acid

The titration of a polyprotic base such as sodium carbonate with a strong acid such as hydrochloric acid results in two equivalence points on the titration curve. At the first equivalence point, the carbonate ions in the base are completely converted to bicarbonate ions. The second equivalence point corresponds to the complete conversion of bicarbonate ions to carbonic acid, which dissociates into carbon dioxide and water. The region before the first equivalence point corresponds to the...
Qualitative Analysis03:46

Qualitative Analysis

For solutions containing mixtures of different cations, the identity of each cation can be determined by qualitative analysis. This technique involves a series of selective precipitations with different chemical reagents, each reaction producing a characteristic precipitate for a specific group of cations. Metal ions within a group are further separated by varying the pH, heating the mixture to redissolve a precipitate, or adding other reagents to form complex ions.
For instance, group IV...
Solvating Effects02:12

Solvating Effects

An understanding of the solvating effect helps rationalize the relation between solvation and acidity of the compound. In addition, this also explains the relative stability of conjugate bases for compounds with different pKa values. This lesson details, in-depth, the principle of solvating effects. The strength of an acid and the stability of its corresponding conjugate base are determined using pKa values. This observed relationship is a consequence of solvation, which is the interaction...

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Synthesis of Ionic Liquid Based Electrolytes, Assembly of Li-ion Batteries, and Measurements of Performance at High Temperature
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Synthesis of Ionic Liquid Based Electrolytes, Assembly of Li-ion Batteries, and Measurements of Performance at High Temperature

Published on: December 20, 2016

p-Nitrophenolate: a probe for determining acid strength in ionic liquids.

Francesca D'Anna1, Sandra La Marca, Renato Noto

  • 1Dipartimento di Chimica Organica E. Paterno, Università degli Studi di Palermo, Viale delle Scienze-Parco d'Orleans II, 90128 Palermo, Italy. fdanna@unipa.it

The Journal of Organic Chemistry
|January 28, 2009
PubMed
Summary

Protonation equilibrium was studied in ionic liquids using spectrophotometric titration. Carboxylic acids showed less dissociation in ionic liquids compared to water, influenced by both the ionic liquid and acid properties.

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Functional Characterization of Na+/H+ Exchangers of Intracellular Compartments Using Proton-killing Selection to Express Them at the Plasma Membrane
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Area of Science:

  • Physical Chemistry
  • Electrochemistry
  • Solution Chemistry

Background:

  • Room-temperature ionic liquids (RTILs) offer unique solvent properties.
  • Establishing acidity scales in RTILs is crucial for chemical applications.
  • The behavior of weak acids in RTILs differs from aqueous solutions.

Purpose of the Study:

  • To determine an acidity scale for room-temperature ionic liquid solutions.
  • To investigate the protonation equilibrium of sodium p-nitrophenolate in specific ionic liquids.
  • To compare acid dissociation in ionic liquids versus aqueous solutions.

Main Methods:

  • Spectrophotometric titration was employed to study protonation.
  • Sodium p-nitrophenolate was used as the indicator species.
  • Various carboxylic acids with differing strengths were utilized.

Main Results:

  • Carboxylic acids exhibited lower dissociation in the studied ionic liquids ([bm(2)im][NTf(2)] and [bmpyrr][NTf(2)]) compared to water.
  • The protonation equilibrium was sensitive to the specific ionic liquid used.
  • Acid dissociation was influenced by the interplay between the ionic liquid and the carboxylic acid structure.

Conclusions:

  • The study provides insights into acidity in RTILs.
  • Carboxylic acid behavior in ionic liquids is distinct from aqueous media.
  • Interactions between ionic liquids and solutes significantly affect acid-base equilibria.