相关实验视频
Updated: Jul 2, 2026
10:33
Generation of Alginate Microspheres for Biomedical Applications
Published on: August 12, 2012
20.9K
酸属性和化度对酸珠网状和大小的影响:一种现象学方法
Chanez Bennacef1,2, Stéphane Desobry1, Jordane Jasniewski1
1Université de Lorraine, Laboratoire d'Ingénierie des Biomolécules (LIBio), ENSAIA, 54000 Nancy, France.
Polymers
|October 28, 2023
概括
这项研究利用电振挤出优化了酸盐珠子的生产. 化度,酸盐分子量和M/G比率显著影响珠子的大小,使得量身定制的材料性能.
科学领域:
- 生物材料工程 生物材料工程
- 聚合物科学 聚合物科学
- 化学工程是化学工程的重要组成部分.
背景情况:
- 酸珠是用于药物输送和组织工程的多功能生物材料.
- 控制酸盐珠子的大小对于优化其在各种应用中的性能至关重要.
- 电振挤出提供了一种精确的方法,用于酸盐珠子的形成.
研究的目的:
- 调查影响酸盐珠子尺寸的关键因素,通过电振挤出生产.
- 建立酸盐网状和珠子形成的现象学模型.
- 为特定应用量身定制酸盐材料提供见解.
主要方法:
- 使用两种酸盐类型 (AlgLF和AlgP) 通过电振挤出生产酸盐珠.
- 使用NMR和SEC-MALS对酸盐的特性进行表征,包括曼酸盐/酸盐 (M/G) 的比率和分子量.
- 过程参数的系统变化:化度,流量和振动频率.
- 酸盐网状化过程的数学建模.
主要成果:
- 化度是影响珠子大小的主要因素,度较高会产生较小的珠子.
- 酸的分子量和M/G比率也显著影响了珠子的大小;较高的分子量和较低的G-块含量导致珠子更小.
- 流速和振动频率影响了珠子的大小,而酸盐溶液老化的影响最小.
- 一个数学方程被开发出来,用于模拟酸盐网膜.
结论:
- 酸盐珠子的大小可以通过电振挤出控制,通过操纵离子度,酸盐分子量和M / G比率来控制.
- 这些发现为优化基于酸盐的材料用于各种应用提供了基础.
- 一个现象学模型有助于理解和定制定制的酸盐材料的凝过程.
相关概念视频
02:41pH Scale
Hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes. Two different solutions can differ in their hydronium or hydroxide ion concentrations by a million, billion, or even trillion times. A common means of...
03:05Acid Strength and Molecular Structure
Binary Acids and Bases
In the absence of any leveling effect, the acid strength of binary compounds of hydrogen with nonmetals (A) increases as the H-A bond strength decreases down a group in the periodic table. For group 17, the order of increasing acidity is HF < HCl < HBr < HI. Likewise, for group 16, the order of increasing acid strength is H2O < H2S < H2Se < H2Te. Across a row in the periodic table, the acid strength of binary hydrogen compounds increases with increasing...
In the absence of any leveling effect, the acid strength of binary compounds of hydrogen with nonmetals (A) increases as the H-A bond strength decreases down a group in the periodic table. For group 17, the order of increasing acidity is HF < HCl < HBr < HI. Likewise, for group 16, the order of increasing acid strength is H2O < H2S < H2Se < H2Te. Across a row in the periodic table, the acid strength of binary hydrogen compounds increases with increasing...
03:24Common Ion Effect
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Châtelier’s principle. Consider the dissolution of silver iodide:
02:34Molecular Structure and Acidity
An acid can be deprotonated to form a conjugate base or an anion. If the produced anion is more stable, then the acid is stronger. On the contrary, if the anion is unstable, then the acid is weaker. Hence, to determine the acidity of the compound, the stability of its conjugate base is studied using various factors.
The size effect explains the change in atomic size on acidity. When comparing the acids formed from elements that belong to the same column in the periodic table, their atomic sizes...
The size effect explains the change in atomic size on acidity. When comparing the acids formed from elements that belong to the same column in the periodic table, their atomic sizes...
01:19Ionic Strength: Effects on Chemical Equilibria
The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary cation—the calcium...
In this solution, the primary cation—the calcium...
01:17Factors Affecting Activity Coefficient
The extended Debye-Hückel equation indicates that the activity coefficient of an ion in an aqueous solution at 25°C depends on three partially interdependent properties: the ionic strength of the solution, the charge of the ion, and the ion size.
The activity coefficient value for an ion is close to one when the solution has almost zero ionic strength, i.e., when the solution shows close to ideal behavior. As the ionic strength of the solution increases from 0 to 0.1 mol/L, a decrease in the...
The activity coefficient value for an ion is close to one when the solution has almost zero ionic strength, i.e., when the solution shows close to ideal behavior. As the ionic strength of the solution increases from 0 to 0.1 mol/L, a decrease in the...