Biosorption of cesium（Ⅰ） from aqueous solution by a novel exopolymers secreted from Pseudomonas fluorescens C-2： Equilibrium and kinetic studies

The biosorption characteristics of Cs(I) ions from aqueous solution using exopolymers (PFC02) produced from Pseudomonas fluorescens C-2 were investigated as a function of pH, biosorbent dosage, contact time and initial concentration. pH played a major role in the adsorption process, and the optimum pH for the removal of Cs(I) was 8.0. Langmuir, Freundlich and Dubinin-Radushkevich (D-R) models were applied to describe the biosorption isotherm of the Cs(I) ions by PFC02. The Lagergren first-order, pseudo second-order kinetic and intraparticle diffusion models were used to test the kinetic data. Langmuir model and D-R model fitted the equilibrium data better than the Freundlich isotherm. The monolayer adsorption capacities of PFC02 as obtained from Langmuir isotherm at 25°C was found to be 32.63 mg/g. From the D-R isotherm model, the mean free energy was calculated as 26.73 kJ/mol, indicating that the biosorption of cesium was chemisorption. The biosorption process was rapid, and the kinetic rates were best fitted to the pseudo second-order model, which indicated the biosorption process operated through chemisorption mechanism. FT-IR analysis of PFC02 showed the possible functional groups responsible for cesium adsorption were hydroxyl, carboxyl, carbonyl and sulphonate groups. SEM analysis showed the porous structure of the material while EDX analysis confirmed the adsorption of Cs(I) on PFC02. Cesium adsorbed onto the PFC02 could be desorbed efficiently using 1 mol/L HNO3, and the enrichment factor was 50.0. Furthermore, PFC02 could be reused five times with only about 8.25% regeneration loss. The developed method was successfully utilized for the removal of Cs(I) ions from aqueous solution.     

四钛酸钾晶须对亚甲基蓝吸附性能研究

利用四钛酸钾晶须作为吸附剂,研究了亚甲基蓝在其上的吸附行为,考察了吸附体系pH值、吸附剂用量、吸附时间对其吸附效果的影响.实验结果表明,四钛酸钾晶须对亚甲基蓝有较强的吸附力,得到的吸附等温线能较好的符合Freundlich方程,其R2都能达到0.991以上,吸附动力学可以用拟二级动力学模型描述.在碱性范围内四钛酸钾晶须...     

改性硅藻土对三种有机染料的吸附作用研究

以天然硅藻土分别负载十六烷基三甲基溴化铵(CTMAB)、四甲基溴化铵(TMAB)和壳聚糖,制得一系列改性硅藻土,研究了改性硅藻土吸附水中的阴离子染料(活性红120)、阳离子染料(亚甲基蓝)、酸性染料(玫瑰红B)的适宜条件及吸附机理.结果表明,天然硅藻土对亚甲基蓝、四甲基溴化铵改性硅藻土对玫瑰红B和壳聚糖改性硅藻土对活性红120的饱和吸附量分别为51.15、49.56、56.64mg.L-1,效果良好,可被直接利用.延长吸附时间、增大吸附剂用量、控制溶液的pH值(<6)都能提高改性硅藻土吸附剂的吸附效果;3种染料在各自吸附剂上的平衡吸附量Qe与平衡浓度Ce之间的关系均符合Freundlich等温吸附方程,表明改性硅藻土吸附染料以分配作用、弱的溶质吸收为主.改性剂的引入可以改变硅藻土的表面电性,从而对不同类型染料的吸附能力产生不同影响.     

活性污泥对病毒的生物吸附特性

针对污水处理过程中可能存在的病原微生物对人体健康的风险,以f2噬菌体为模型病毒,采用静态吸附方法,研究病毒在活性污泥上的生物吸附特性及其影响因素,以期了解病毒在活性污泥处理系统中固液两相体系的分配规律.结果表明,活性污泥对病毒的吸附速率快,吸附量大,在120 min时即能达到吸附平衡,平衡吸附率高达96%以上,对病毒的去除效果较为理想;该吸附符合Freundlich吸附等温式,且吸附率随着病毒浓度的增加而呈现出下降趋势;另外,pH值、金属阳离子浓度及有机物浓度均可显著影响病毒在活性污泥上的吸附.     

挥发性氯代烃在湿润土壤中的平衡吸附研究

吸附是挥发性氯代烃(volatile chlorinated hydrocarbons,VCHs)赋存于土壤的主要机制之一.开展动态吸附实验,研究了4种常见VCHs污染物在我国8种典型土壤中的吸附平衡关系.结果表明,土壤在干燥条件下对VCHs气体的吸附能力要远大于湿润条件,且随含水率的升高吸附能力急剧下降,在含水率达到10%以后土壤吸附量趋于稳定.湿润土壤对三氯乙烯(TCE)、四氯乙烯(PCE)、1,1,1-三氯乙烷(MC)气体的吸附等温线符合Henry型吸附等温式,而1,1,2-三氯乙烷(1,1,2-TCA)符合Freundlich模型.VCHs在湿润土壤中的吸附量总体上与土壤有机碳(soil organic carbon,SOC)含量呈正相关,且受SOC类型和化合物极性影响较大.弱极性的TCE、PCE在土壤中的吸附能力与SOC含量呈严格正相关,而极性的MC、1,1,2-TCA在黑土等高碳土壤中不仅与SOC含量有关,还受到SOC物质组成的影响.建立了TCE和PCE在湿润土壤中的平衡吸附量预测模型,预测值与实测值相关性良好(n=80,R2=0.98).     

镁-钙羟基磷灰石吸附剂对水中Pb2+的去除

选择Mg2+为掺杂离子,通过溶胶-凝胶法制备了不同比例的镁-钙羟基磷灰石吸附剂,研究其对水溶液中Pb~(2+)的去除特性和过程机制.结果表明,吸附剂表面以羟基磷铅矿化合物[Pb10(PO4)6(OH)2]为主,其晶体结构由短棒状转变为针状结构;在温度25℃,p H为5时,镁-钙羟基磷灰石吸附Pb~(2+)在720 min内达到平衡,吸附剂的最佳投加量为0. 6 g·L-1,最大吸附量为813. 17 mg·g-1;热力学实验结果:ΔGθ0、ΔSθ 0和ΔHθ 0,表明镁-钙羟基磷灰石吸附Pb~(2+)的过程是自发的吸热、熵增的过程,升温有利于吸附;吸附过程符合伪二级动力学方程,Langmuir吸附模型能更好地描述等温吸附行为;材料表征与吸附实验分析表明,表面络合与溶解-沉淀是镁-钙羟基磷灰石去除Pb~(2+)的主要机制.     

ANAMMOX颗粒污泥吸附氨氮特性及其影响因素

为了解析ANAMMOX颗粒污泥对氨氮的吸附特性及机理,分别考察了不同初始氨氮浓度和污泥浓度下的ANAMMOX颗粒污泥吸附氨氮特性,以及温度、pH、盐度和金属阳离子对氨氮吸附的影响;并采用了吸附等温式、动力学和热力学对吸附过程进行解析.结果表明,ANAMMOX颗粒污泥对氨氮的吸附在20min左右基本达到吸附平衡,吸附容量随着氨氮初始浓度的增加而增加,随ANAMMOX颗粒污泥浓度的升高而减少.低温有利于ANAMMOX颗粒污泥对氨氮的吸附,其最佳pH为7.0.盐度和金属阳离子显著影响ANAMMOX颗粒污泥对氨氮的吸附,在NaCl浓度为5g/L时,吸附作用已不明显.在质量浓度相同的条件下,Fe³⁺对吸附作用抑制最强,Mg²⁺与Ca²⁺次之,而Cu²⁺相对最弱.ANAMMOX颗粒污泥吸附氨氮过程更符合Freundlich等温式,吸附过程符合准二级动力学模型,并且是由表层扩散和内部扩散共同作用的结果.热力学研究表明,该吸附过程是一个自发的放热过程.     

Ackee apple (Blighia sapida) seeds: a novel adsorbent for the removal of Congo Red dye from aqueous solutions

The ability of ackee apple (AA) seeds to remove Congo Red (CR) dye from aqueous solution was investigated. AA was characterised using thermo gravimetric analyser, scanning electron microscopy, Braunauer Emmett Teller, pH_pzc, elemental analysis and Boehm titration. The effects of operational parameters such as adsorbent dosage, contact time, initial dye concentration and solution pH were studied in a batch system. pH has a profound influence on the adsorption process. Maximum dye adsorption was observed at pH 3.0. The reaction was fast, reaching equilibrium in 90 min. Adsorption data were best described by Langmuir isotherm and the pseudo-second-order kinetic model with a maximum monolayer coverage of 161.89 mg·g^?1. Both boundary layer and intraparticle diffusion mechanisms were found to govern the adsorption process. Thermodynamic parameters such as standard free energy change (Δ G ⁰), standard enthalpy change (Δ H ⁰), and standard entropy change (Δ S ⁰) were studied. Values of Δ G ⁰ varied between?30.94 and?36.56 kJ·mol^?1, Δ H ⁰ was 25.61 kJ·mol^?1, and Δ S ⁰ was 74.84 kJ·mol^?1·K^?1, indicating that the removal of CR from aqueous solution by AA was spontaneous and endothermic in nature. Regeneration and reusability studies were carried out using different eluents. AA gave the highest adsorption efficiency up to four cycles when treated with 0.3 M HCl. AA was found to be an effective adsorbent for the removal of CR dye from aqueous solution.     

Adsorptive removal of a synthetic textile dye using cocoa pod husks

The adsorption of a synthetic textile dye (Remazol Brilliant Black Reactive) on cocoa pod husk-based activated carbon was investigated in batch process. The adsorbent prepared was characterized by gas adsorption surface analysis (Brunauer Emmett Teller, BET), scanning electron microscopy, and Fourier transform infrared spectroscopy. The effects of initial dye concentration, contact time, solution temperature, and solution pH were evaluated. Equilibrium data were fitted to Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherm models, the first being the best with maximum monolayer coverage of 111?mg?g^?1. Kinetic data were fitted into pseudo-first-order, pseudo-second-order, intraparticle diffusion, and Elovich models; the pseudo second-order model provided the best correlation. Maximum adsorption was observed at pH 7. Standard free energy, standard enthalpy, and standard entropy were also calculated. The adsorption interaction was found to be endothermic and spontaneous. Both the mean free energy of adsorption and the activation energy show that the mechanism is by physisorption.     

Preparation and characterization of calcium alginate-based composite adsorbents for the removal of Cd,Hg, and Pb ions from aqueous solution

Composite adsorbent materials containing calcium alginate, clinoptilolite, and coal-derived humic acid were prepared. Humic acid (HA), clinoptilolite (CL), alginate (AL), alginate-entrapped humic acid (AL/HA), clinoptilolite (AL/CL), and humic acid/clinoptilolite (AL/HA/CL) samples were characterized. The effectiveness of the samples as adsorbents for the removal of cadmium (Cd), mercury (Hg), and lead (Pb) were studied in a series of batch-adsorption experiments. For the AL, AL/HA, AL/CL, and AL/HA/CL adsorbents, uptake versus time data were evaluated using two kinetic models, a linear and a non-linear pseudo-first-order and a pseudo-second-order model. The data for each metal ion on all adsorbents showed good correspondence with the pseudo-second-order kinetic model. The equilibrium data were fitted to Langmuir, Freundlich, Dubinin–Radushkevich, and Temkin isotherm models. The results show that a non-linear method seems more appropriate for obtaining isotherm parameters. The non-linear Freundlich and Langmuir models for Pb and Hg produced a best fit with high R ² value (0.99). For HA adsorbent, the equilibrium data for Cd removal better fit to the non-linear Dubinin–Radushkevich isotherm.