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Basicity of Aliphatic Amines01:21

Basicity of Aliphatic Amines

6.2K
Amines can behave as Brønsted–Lowry bases by accepting a proton from the acid to form corresponding conjugate acids. Due to a lone pair of nonbonding electrons, aliphatic amines can also act as Lewis bases by forming a covalent bond with an electrophile.
To measure the basicity of amines, two conventions are generally used. The first defines Kb as the basicity constant for the deprotonation reaction of water by the amine, as presented in Figure 1. Conventionally, lower Kb indicates...
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Extraction: Effects of pH00:53

Extraction: Effects of pH

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Consider a neutral form of an amine, B, with a partition coefficient, K, in a liquid mixture containing organic and aqueous phases. The pH of the aqueous phase affects the charge on acidic and basic solutes, and the charged form is usually more soluble in the aqueous phase. Suppose the conjugate acid form of the amine is soluble only in the aqueous phase while the base form is soluble in both phases. Then the distribution coefficient, D, can be given as the ratio of amine concentration in the...
739
Titration in Nonaqueous Solvents01:16

Titration in Nonaqueous Solvents

1.0K
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,...
1.0K
Titration of Polyprotic Acids with a Strong Base01:23

Titration of Polyprotic Acids with a Strong Base

2.0K
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...
2.0K
Weak Base Solutions03:21

Weak Base Solutions

23.2K
Some compounds produce hydroxide ions when dissolved by chemically reacting with water molecules. In all cases, these compounds react only partially and so are classified as weak bases. These types of compounds are also abundant in nature and important commodities in various technologies. For example, global production of the weak base ammonia is typically well over 100 metric tons annually, being widely used as an agricultural fertilizer, a raw material for chemical synthesis of other...
23.2K
Titration of a Polyprotic Acid02:08

Titration of a Polyprotic Acid

97.6K
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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Author Spotlight: Standardizing the Development of Amine-Based Silica Composites as CO2 Adsorbents for Direct Air Capture
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Multiobjective Evaluation of Amine-Based Absorbents for SO2 Capture Process Using the pK a Mathematical Model.

Dongliang Wang1,2, Jiangpeng Xie1,2, Guixian Li1,2

  • 1School of Petrochemical Engineering, Lanzhou University of Technology, Lanzhou, Gansu 730050, China.

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|January 31, 2022
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Summary
This summary is machine-generated.

Screening amine-based absorbents for sulfur dioxide (SO2) capture is crucial. This study models SO2 cyclic absorption capacity and desorption heat, finding a balance between capacity and energy is key for effective flue gas treatment.

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Area of Science:

  • Environmental Chemistry
  • Chemical Engineering
  • Materials Science

Background:

  • Efficient sulfur dioxide (SO2) capture from flue gas requires high-performance, low-energy absorbents.
  • Amine-based absorbents are critical for SO2 removal, but their performance varies.
  • Screening effective absorbents necessitates understanding their absorption capacity and energy requirements.

Purpose of the Study:

  • To screen high-efficiency, low-energy consumption absorbents for SO2 capture.
  • To establish a quantitative relationship between absorbent properties and performance metrics.
  • To guide the development of advanced amine-based SO2 capture systems.

Main Methods:

  • Quantum chemical calculations to determine acidity coefficient (pKa) of five diamines: ethylenediamine (EDA), piperazine (PZ), 1-(2-hydroxyethyl)piperazine (HEP), 1,4-bis(2-hydroxyethyl)piperazine (DIHEP), and 1-(2-hydroxyethyl)-4-(2-hydroxypropyl)piperazine (HEHPP).
  • Mathematical modeling to predict SO2 cyclic absorption capacity per amine (αc) based on solution electroneutrality.
  • Mathematical modeling using the van't Hoff equation to predict desorption reaction heat (Qdes), with results verified against experimental data.

Main Results:

  • Calculated pKa values correlate with both SO2 cyclic absorption capacity (αc) and desorption reaction heat (Qdes).
  • The order of αc is EDA > PZ > HEHPP > HEP > DIHEP, while the order of Qdes is EDA > PZ > HEHPP > DIHEP > HEP.
  • Multiobjective analysis indicates that optimizing αc without considering Qdes is not advisable; compound quaternary systems offer wider αc ranges than single ternary systems.

Conclusions:

  • The study provides a quantitative framework for screening amine-based SO2 absorbents.
  • Balancing absorption capacity and desorption energy is essential for efficient SO2 capture.
  • Development of compound quaternary system absorbents is a promising direction for future research.