共查询到19条相似文献,搜索用时 109 毫秒
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根据林邦副反应思想,分别得到一元强碱滴定一元强酸和一元强碱滴定一元弱酸的精确滴定曲线为一元二次和一元三次方程.利用Origin软件解析酸碱滴定曲线方程,并以滴定分数为横坐标,pH为纵坐标绘制滴定曲线. 相似文献
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为了研究平衡的变化规律,我们曾撰文介绍滴定曲线与滴定过程型体分布图并联的方法。本文将讨论滴定曲线与滴定液的缓冲容量曲线和敏锐指数曲线并联研究平衡的方法。理论推导 1.强碱滴定酸参照文献[2]可以得出,以浓度为C的NaOH溶液滴定浓度为C_0、体积为V_0的n元酸H_nB,当加入NaOH V时滴定曲线方程为: 相似文献
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本文首先利用物料平衡和林邦副反应思想分别推导出n1=n2和n1≠n2两种情况时的氧化还原滴定曲线方程,然后应用Origin软件对所推导的不同曲线方程进行解析,建立起以溶液电势E为因变量,滴定分数a为自变量的函数关系,并绘制其滴定曲线。 相似文献
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为了改造氧化还原滴定分析方法的标度,从而逐步建立统一的滴定分析标度计算式,提出了相对电子浓度Re-的概念,基于此发展了以p Re-为监测标度的氧化还原滴定方法新理论。该理论描述了氧化还原半反应的平衡,推导了氧化还原滴定标度p Re-的计算通式,探索了该标度在滴定过程中的一般变化规律,重新梳理了指示剂的指示原理。以Ce4+滴定Fe3+溶液为例,演绎了如何简单绘制滴定曲线、计算滴定突跃范围、判断可否直接准确滴定,讨论了氧化还原反应条件平衡常数Kτ?’的大小对滴定分析的影响。 相似文献
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以林邦副反应思想为基础,用质子条件式PBE、物料平衡式MBE、滴定分数和条件稳定常数等知识推导出一元强碱滴定一元弱酸溶液的林邦滴定曲线方程,并用滴定曲线方程讨论了滴定开始至化学计量点时任意一点p H的计算。 相似文献
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滴定曲线是滴定分析原理的重要内容。它显示了滴定过程中平衡体系性质的变化,可以获知化学计量点和滴定突跃信息,从而指导准确滴定判别或指示剂的选择。滴定曲线方程是滴定过程中体系的某种性质X(例pH)与滴定分数a(或滴定剂体积V)的关系方程,解析方程可获得函数X=f(a)的表达式。对一些较复杂的体系,推导函数X=f(a)较困难,但多数情况下反函数a=g(X)的推导更容易,表达式也更简洁。本文对酸碱、配位、氧化还原和沉淀滴定曲线方程进行了系统总结,并对不同情况下的函数X=f(a)或反函数a=g(X)进行了推导,拓展了教材内容。根据函数关系,在Origin中利用其函数绘图功能可直接绘制出滴定曲线,不用先生成数据点再绘图,方便快捷。用反函数绘图时增加数据点即可获得高精度的滴定曲线,可直接从滴定曲线上查找化学计量点和滴定突跃信息。 相似文献
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武汉大学主编的《分析化学》(第 4版 ) [1] 是一部面向 2 1世纪的教材 ,又是普通高等教育“九五”国家级重点教材 ,它的出版标志着我国化学基础学科发展的一个新阶段 ,也是分析化学教育第一线的教师们翘首企盼的大事。该部教材有了许多重大的进步 ,例如用滴定曲线方程统一处理各类滴定曲线 ;将分析试样的制备和分解合并到定量分析概论一章 ;增加了分离和富集方法一章的内容等 ,这些进步使得定量分析课程设置更为合理和科学。另外 ,新教材的印刷质量之精美 ,也是以往教材无法比拟的。对编者“树立精品意识”的观念应该表示赞赏 ,这毕竟是一部… 相似文献
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A titration method has been developed to analyze acid mixtures, in which the pK values differed by 0.5 to 1 pH units. Instead of the use of equivalence points a buffer capacity curve is numerically derived from the titration curve resulting in a presentation similar to chromatograms and spectra. The consumption of the NaOH titrant is determined within pH intervals of 0.2-0.6 units around the pK values of the components. The buffer capacity measured is expressed as the consumption of NaOH over the pH interval. The amounts of compounds are found from these results using simple models of chemometrics. The method has been applied to a mixture of formic and acetic acids with concentrations of 0-3 mmol/20 ml with an error of 0-0.05 mmol. Furthermore a curve-fitting method based on a theoretical equation of buffer capacity can be applied with an error slightly larger than with the previous method. In this case, the pK values were also computed. For titrations beyond the pH range 4-10, the buffer capacity of water has to be subtracted from the titration results. The whole procedure requires including the computations about 3-6 min. 相似文献
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A titration method has been developed to analyze acid mixtures, in which the pK values differed by 0.5 to 1 pH units. Instead of the use of equivalence points a buffer capacity curve is numerically derived from the titration curve resulting in a presentation similar to chromatograms and spectra. The consumption of the NaOH titrant is determined within pH intervals of 0.2–0.6 units around the pK values of the components. The buffer capacity measured is expressed as the consumption of NaOH over the pH interval. The amounts of compounds are found from these results using simple models of chemometrics. The method has been applied to a mixture of formic and acetic acids with concentrations of 0–3 mmol/20 ml with an error of 0–0.05 mmol. Furthermore a curve-fitting method based on a theoretical equation of buffer capacity can be applied with an error slightly larger than with the previous method. In this case, the pK values were also computed. For titrations beyond the pH range 4–10, the buffer capacity of water has to be subtracted from the titration results. The whole procedure requires including the computations about 3–6 min. 相似文献
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非水滴定法测定酰胺缩醛 总被引:3,自引:0,他引:3
对非水滴定酰胺缩醛的溶剂、滴定剂和指示剂进行了选择试验,用HCl甲醇标准液进行滴定,通过电位滴定曲线或甲基橙指示剂可以准确的确定滴定终点,方法简便,结果准确。 相似文献
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Morel JP Marmier N Hurel C Morel-Desrosiers N 《Journal of colloid and interface science》2006,298(2):773-779
Sorption reactions on natural or synthetic materials that can attenuate the migration of pollutants in the geosphere could be affected by temperature variations. Nevertheless, most of the theoretical models describing sorption reactions are at 25 degrees C. To check these models at different temperatures, experimental data such as the enthalpies of sorption are thus required. Highly sensitive microcalorimeters can now be used to determine the heat effects accompanying the sorption of radionuclides on oxide-water interfaces, but enthalpies of sorption cannot be extracted from microcalorimetric data without a clear knowledge of the thermodynamics of protonation and deprotonation of the oxide surface. However, the values reported in the literature show large discrepancies and one must conclude that, amazingly, this fundamental problem of proton binding is not yet resolved. We have thus undertaken to measure by titration microcalorimetry the heat effects accompanying proton exchange at the alumina-water interface at 25 degrees C. Based on (i) the surface sites speciation provided by a surface complexation model (built from acid-base titrations at 25 degrees C) and (ii) results of the microcalorimetric experiments, calculations have been made to extract the enthalpic variations associated respectively to first and second deprotonation of the alumina surface. Values obtained are deltaH1 = 80+/-10 kJ mol(-1) and deltaH2 = 5+/-3 kJ mol(-1). In a second step, these enthalpy values were used to calculate the alumina surface acidity constants at 50 degrees C via the van't Hoff equation. Then a theoretical titration curve at 50 degrees C was calculated and compared to the experimental alumina surface titration curve. Good agreement between the predicted acid-base titration curve and the experimental one was observed. 相似文献
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Makowska J Bagiñska K Makowski M Jagielska A Liwo A Kasprzykowski F Chmurzyñski L Scheraga HA 《The journal of physical chemistry. B》2006,110(9):4451-4458
We compared the ability of two theoretical methods of pH-dependent conformational calculations to reproduce experimental potentiometric titration curves of two models of peptides: Ac-K5-NHMe in 95% methanol (MeOH)/5% water mixture and Ac-XX(A)7OO-NH2 (XAO) (where X is diaminobutyric acid, A is alanine, and O is ornithine) in water, methanol (MeOH), and dimethyl sulfoxide (DMSO), respectively. The titration curve of the former was taken from the literature, and the curve of the latter was determined in this work. The first theoretical method involves a conformational search using the electrostatically driven Monte Carlo (EDMC) method with a low-cost energy function (ECEPP/3 plus the SRFOPT surface-solvation model, assumming that all titratable groups are uncharged) and subsequent reevaluation of the free energy at a given pH with the Poisson-Boltzmann equation, considering variable protonation states. In the second procedure, molecular dynamics (MD) simulations are run with the AMBER force field and the generalized Born model of electrostatic solvation, and the protonation states are sampled during constant-pH MD runs. In all three solvents, the first pKa of XAO is strongly downshifted compared to the value for the reference compounds (ethylamine and propylamine, respectively); the water and methanol curves have one, and the DMSO curve has two jumps characteristic of remarkable differences in the dissociation constants of acidic groups. The predicted titration curves of Ac-K5-NHMe are in good agreement with the experimental ones; better agreement is achieved with the MD-based method. The titration curves of XAO in methanol and DMSO, calculated using the MD-based approach, trace the shape of the experimental curves, reproducing the pH jump, while those calculated with the EDMC-based approach and the titration curve in water calculated using the MD-based approach have smooth shapes characteristic of the titration of weak multifunctional acids with small differences between the dissociation constants. Nevertheless, quantitative agreement between theoretically predicted and experimental titration curves is not achieved in all three solvents even with the MD-based approach, which is manifested by a smaller pH range of the calculated titration curves with respect to the experimental curves. The poorer agreement obtained for water than for the nonaqueous solvents suggests a significant role of specific solvation in water, which cannot be accounted for by the mean-field solvation models. 相似文献