塑料在变性和多孔介质中的运动:离子强度和表面粗度的作用
Yang Zhou1, Shoichiro Hamamoto2, Takuhei Yamasaki1
1Graduate School of Agricultural and Life Science, The University of Tokyo, Japan.
Journal of contaminant hydrology
|February 13, 2026
概括
离子强度会影响多孔介质中的合体运输,增加附着度. 表面粗性出乎意料地提高了和条件下合体的移动性,但在不和条件下增加了附着性.
科学领域:
- 环境科学 环境科学
- 合体和表面科学科学
- 地质化学 地质化学
背景情况:
- 在多孔介质中的合体沉积对于污染物运输至关重要.
- 了解诸如离子强度和表面粗度等因素是预测合体行为的关键.
- 现有的模型往往简化了收集器表面的复杂相互作用.
研究的目的:
- 为了研究离子强度和收集器表面粗度对合物沉积机制的影响.
- 阐明物理粗性和化学因素在和和不和多孔介质中的作用.
- 在不同的实验条件下评估合物保留和附着.
主要方法:
- 实验使用定制的柱子设置,使用光滑和粗的 (HF蚀刻) 玻璃珠.
- 不同的离子强度 (IS) 从1-100mM.
- 通过柱体解剖量化附着的合物,并分析合物释放配置文件.
主要成果:
- 增加IS减少移动合体和增强附着性,与DLVO理论和正电荷异质性保持一致.
- 随着IS的增加,体保留概况从非线性转变为线性,表明过渡到有利的附着.
- 不和条件增加了合体的保留和附着,由拦截和空气-水-固体接口驱动.
- 表面粗性在和条件下意外增强了合体的移动性,但在不和条件下增加了紧密的附着性.
结论:
- 体运输是由离子强度,表面粗度和和水平之间的复杂相互作用来控制的.
- 表面粗度对合体沉积的影响取决于环境,根据和和粗度的尺度而有所不同.
- 这些发现有助于更好地理解环境合物在多孔介质中的运输和沉积机制.
关键词:
附加物 附加物 附加物体体是一种体.这里是ISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISISIS释放 释放 释放 释放粗性 粗性 粗性不和的状态 不和的状态
相关概念视频
01:12Ionic Strength: Overview
3.1K
The ionic strength of a solution is a quantitative way of expressing the total electrolyte concentration of a solution. This concept was first introduced in 1921 by two American physical chemists, Gilbert N. Lewis and Merle Randall, while describing the activity coefficient of strong electrolytes. During the calculation of ionic strength (I or μ), all the cations and anions are considered. However, the concentration (c) of an ion with a greater charge number (z) has a greater contribution...
3.1K
01:19Ionic Strength: Effects on Chemical Equilibria
2.8K
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...
In this solution, the primary...
2.8K
00:42Ionic Bonds
132.5K
Overview
When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.
Opposing Charges Hold Ions Together in Ionic Compounds
Ionic bonds are reversible electrostatic interactions between ions...
When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.
Opposing Charges Hold Ions Together in Ionic Compounds
Ionic bonds are reversible electrostatic interactions between ions...
132.5K
02:54Molecular and Ionic Solids
20.3K
Crystalline solids are divided into four types: molecular, ionic, metallic, and covalent network based on the type of constituent units and their interparticle interactions.
Molecular Solids
Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...
Molecular Solids
Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...
20.3K
01:59Solution Equilibrium and Saturation
22.3K
Imagine adding a small amount of sugar to a glass of water, stirring until all the sugar has dissolved, and then adding a bit more. You can repeat this process until the sugar concentration of the solution reaches its natural limit, a limit determined primarily by the relative strengths of the solute-solute, solute-solvent, and solvent-solvent attractive forces. You can be certain that you have reached this limit because, no matter how long you stir the solution, undissolved sugar remains. The...
22.3K
03:10Ionic Radii
33.9K
Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it is smaller than the atom from which it is derived. For example, the covalent radius of an aluminum atom (1s22s22p63s23p1) is 118 pm, whereas the ionic radius of an Al3+ (1s22s22p6) is 68 pm. As electrons are removed from the outer valence shell, the remaining core electrons occupying smaller shells experience a greater effective nuclear...
33.9K