结合的clinoptilolite和Fe(O) OH,以有效地去除Cu(II) 和Pb(II),并增强固体-液体分离
Jennifer N Enemmoh1, David Harbottle1, Muhammad Yusuf2,3
1School of Chemical and Process Engineering, University of Leeds, Leeds, LS2 9JT UK.
概括
这项研究结合了clinoptilolite和铁氧化物,以有效地去除重金属. 双重用途的花剂有效地去除了和铜离子,改善了固体和液体的分离.
科学领域:
- 环境科学 环境科学
- 材料科学 材料科学 材料科学
- 化学工程是化学工程的重要组成部分.
背景情况:
- 重金属 (Pb2+,Cu2+) 的污染对环境构成重大风险.
- 传统的去除方法,如离子交换和沉,都有局限性.
- 开发具有成本效益和效率的花剂对于水资源整治至关重要.
研究的目的:
- 为了研究clinoptilolite和铁氧化物 (FeOOH) 作为双重用途的花剂的结合的协同效应.
- 加强从水溶液中去除 (Pb2+) 和铜 (Cu2+) 离子.
- 评估对固体-液体分离,花特性和脱水性能的影响.
主要方法:
- 使用伪二阶 (PSO) 和朗穆尔模型进行吸附动力学和平衡研究.
- 使用传输电子显微镜 (TEM),扫描电子显微镜 (SEM) 和X射线衍射 (XRD) 进行材料的表征.
- 评估流量大小,结算率,整合和压缩性收益率压力.
主要成果:
- 克林诺皮托利的吸附遵循PSO动力学和兰慕尔异常热,具有Pb2+和Cu2+的高容量.
- 在SEM中,发现了用FeOOH (α-FeOOH/Goethite) 装饰的克林诺皮托利特核.
- 结合的比单独的FeOOH更大,沉积更快,结合更好,增加了脱水.
- 实现了超过98%的Pb2+和Cu2+的去除,超过单独的FeOOH.
结论:
- 与单个组件相比,clinoptilolite-FeOOH组合系统在重金属清除方面提供了更高的性能.
- 增强的花和沉性质显著提高了固体液体分离的效率.
- 这种具有成本效益的双重用途的花剂为工业废水处理提供了一个有前途的解决方案.
更多相关视频
09:23Removal of Trace Elements by Cupric Oxide Nanoparticles from Uranium In Situ Recovery Bleed Water and Its Effect on Cell Viability
Published on: June 21, 2015
9.7K
11:14Two-way Valorization of Blast Furnace Slag: Synthesis of Precipitated Calcium Carbonate and Zeolitic Heavy Metal Adsorbent
Published on: February 21, 2017
12.3K
相关概念视频
Extraction: Advanced Methods
398
Metal ions can be separated from one another by complexation with organic ligands–the chelating agent– to form uncharged chelates. Here, the chelating agent must contain hydrophobic groups and behave as a weak acid, losing a proton to bind with the metal. Since most organic ligands used in this process are insoluble or undergo oxidation in the aqueous phase, the chelating agent is initially added to the organic phase and extracted into the aqueous phase. The metal-ligand complex is...
398
Precipitation and Co-precipitation
1.6K
Precipitation and coprecipitation methods can be used to separate a mixture of ions in a solution. In qualitative inorganic analysis, ions that form sparingly soluble precipitates with the same reagent are separated based on the differences in solubility products. For example, consider the separation of Cu(II) and Fe(II) ions by precipitation as insoluble sulfides. First, copper(II) sulfide is precipitated by the addition of acidic H2S, where the dissociation of H2S is suppressed. Adding H2S...
1.6K
Coagulation
256
Colloidal solids are solid particles suspended in solution. They are usually negatively charged, attracting a compact primary layer of positively charged ions, which attract more counterions to form an electrical double layer. Electrostatic repulsion between the charged double layers prevents the particles from colliding, stabilizing the colloids. These solids are often undesirable because they can contain toxins that are difficult to remove. Coagulation is a technique that helps aggregate and...
256
Colloidal precipitates
478
The high insolubility of some precipitates can result in an unfavorable relative supersaturation. This can lead to colloidal particles with a large surface-to-mass ratio, where adsorption is promoted. For instance, in the precipitation of silver chloride, silver ions are adsorbed on the surface of the colloidal particles, forming a primary layer. This layer attracts ions of opposite charge (such as nitrate ions), forming a diffuse secondary layer of adsorbed ions. This electric double layer...
478
Washing, Drying, and Ignition of Precipitates
816
After filtration, the precipitate is washed to remove coprecipitated impurities and any remaining mother liquor. Colloidal precipitates, such as silver chloride, are washed with an electrolyte (such as dilute nitric acid) to prevent the peptization of the precipitate. In the case of slightly soluble precipitates, the wash solution contains a common ion to reduce solubility. Lead sulfate, which is slightly soluble in water, is washed with dilute sulfuric acid. Similarly, wash solutions may be...
816
Precipitation of Ions
27.5K
Predicting Precipitation
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
27.5K
