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Titration in Nonaqueous Solvents01:16

Titration in Nonaqueous Solvents

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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,...
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Solvating Effects02:12

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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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Bronsted-Lowry Acids and Bases02:58

Bronsted-Lowry Acids and Bases

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The acid-base reaction class has been studied for quite some time. In 1680, Robert Boyle reported traits of acid solutions that included their ability to dissolve many substances, to change the colors of certain natural dyes, and to lose these traits after coming in contact with alkali (base) solutions. In the eighteenth century, it was recognized that acids have a sour taste, react with limestone to liberate a gaseous substance (now known to be CO2), and interact with alkalis to form neutral...
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Lewis Acids and Bases02:33

Lewis Acids and Bases

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In 1923, G. N. Lewis proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond.
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Lewis Acids and Bases02:16

Lewis Acids and Bases

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This lesson delves into Lewis acids and bases in the context of the octet rule for electron-deficient compounds. Here, the concept is discussed, emphasizing the group 13 elements like boron or aluminium. Since group 13 elements possess three valence electrons, they form trivalent compounds with a sextet of electrons and a vacant orbital for the central atom. Consequently, these electron-deficient compounds accept electrons from other species to complete their octet in a chemical reaction. They...
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Leveling Effect and Non-Aqueous Acid-Base Solutions02:11

Leveling Effect and Non-Aqueous Acid-Base Solutions

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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):
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Preparation of Binary and Ternary Deep Eutectic Systems
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Brønsted acidity in deep eutectic solvents and ionic liquids.

Andrew P Abbott1, Sahar S M Alabdullah1, Azhar Y M Al-Murshedi1

  • 1Materials Centre, Department of Chemistry, University of Leicester, Leicester LE1 7RH, UK. apa1@le.ac.uk.

Faraday Discussions
|September 20, 2017
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Summary
This summary is machine-generated.

Proton behavior in deep eutectic solvents (DESs) and ionic liquids was investigated. Organic acids showed slightly lower dissociation in DESs than in water, and water significantly impacted ionic liquid pH.

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Area of Science:

  • Electrochemistry
  • Physical Chemistry
  • Materials Science

Background:

  • Proton behavior in ionic liquids and deep eutectic solvents (DESs) remains poorly understood.
  • Accurate measurement of proton activity in non-aqueous media is challenging.
  • Understanding acid-base properties in these novel solvents is crucial for their application.

Purpose of the Study:

  • To determine acid dissociation constants (pKa) for organic acids in DESs.
  • To investigate the pH behavior of ionic liquids and the influence of water.
  • To explore the development of electrochemical pH sensors for these media.

Main Methods:

  • Titration of DESs with triflic acid using standard pH indicator solutes.
  • Determination of pKIn for bromophenol blue.
  • Measurement of pKIn values for two ionic liquids: [Bmim][BF4] and [Emim][acetate].
  • Development and testing of an electrochemical pH sensor.
  • Analysis of liquid junction potentials between reference electrodes in different DESs.

Main Results:

  • Organic acids exhibited slightly lower dissociation in DESs compared to water (pKa values 0.2–0.5 higher).
  • [Emim][acetate] demonstrated more basic properties than water.
  • Water significantly altered the pH of ionic liquids due to phase partitioning.
  • An electrochemical pH sensor showed a linear response, albeit with a reduced slope compared to aqueous solutions.
  • Liquid junction potential in DESs was pH-dependent.

Conclusions:

  • Established a method for assessing acid-base properties in DESs.
  • Highlighted the significant influence of solvent type and water content on proton behavior.
  • Demonstrated the potential, with limitations, of electrochemical sensors for non-aqueous pH measurements.
  • Provided foundational data for understanding proton activity in ionic liquids and DESs.