一滴汞脉冲极谱法测定矿石中痕量铀

本文报道了在pH5.5的PMBP-醋酸-醋酸钠复合支持电解质中,铀酰离子于E_p=-0.57V(S.C.E.)处产生一灵敏的极谱催化波。本文对铀在此体系中的极谱催化波进行了初步探讨,选择了极谱催化波的底液条件,研究了影响催化电流的因素和波的性质,并用该法测定了矿石中痕量铀。     

半微分极谱分析法

1922年创立极谱学以来,极谱工作者从仪器上作了大量的改进工作。为了克服溶液的内阻产生的电位降和电容电流,消除电解时间对电解电流的影响,Oldham于72年提出了半积分极谱法。75年由Goto在半积分极谱法的基础上提出了半微分极谱法,随后又发展了1.5次和2.5次微分极谱法。这类极谱方法被统称为新极谱法,新极谱法实质上是在电解池输出电流的处理上作了改进。     

半微分极谱分析法

1922年创立极谱学以来,极谱工作者从仪器上作了大量的改进工作。为了克服溶液的内阻产生的电位降和电容电流,消除电解时间对电解电流的影响,Oldham于72年提出了半积分极谱法。75年由Goto在半积分极谱法的基础上提出了半微分极谱法。随后又发展了1.5次和2.5次微分极谱法。这类极谱方法被统称为新极谱法,新极谱法实质上是在电解池输出电流的处理上作了改进。 新极谱理论 Oldham等首先讨论了电流的半积分值,导出半积分值m与去极剂浓度C的关系式。在此基础上Goto等又讨论了电流的半微分值并导出了1.5次2.5次微分值与去极剂浓度C的关系式。     

极谱法同时测定岩石中的微量铀钍

试样经过氧化钠熔融后,用硝酸溶液提取熔块,加入十六烷基三甲基溴化铵（CTMAB）凝聚硅胶,过滤除硅,TBP萃淋树脂分离富集铀钍。在含0．02g／L四丁基碘化铵-4g／L铜铁试剂、pH=5的乙酸-乙酸钠极谱测定体系中同时测定铀钍,铀钍的线性范围为0．001～0．500μg／10mL。本法用于含铀岩石中微量铀钍的同时测定,结果令人满意。     

极谱法在测井中的应用研究

在物探测井工作中,一般的测量参数是电阻率、激化率、磁化率等。测量参数少是造成反演解释多解性的原因之一。本文旨在提出一个新的测井方法──极谱测井,从而提供一个新的测井参数──井液中金属离子的浓度。本文在阐述了极谱法的基本原理的基础上,进行了大量的模拟实验;通过分析实验结果,证实了极谱测并的可行性、有效性和快速性。     

计算极谱法同时测定镉镍的研究

采用普通极谱仪与计算机联机技术,用卡尔曼滤波处理以KSCN为支持电解质的Cd~(2+)和Ni~(2+)混合溶液的示波极谱重叠波。实验表明,极谱可逆波具有较好的加和性,可采用计算极谱方法对多组分(尤其是难以分开的重叠波)进行同时测定。     

矿石中微量铍的极谱测定

铍的极谱测定研究不多,最近已有人报导了用铍试剂Ⅲ测定矿石中微量铍的催化极谱法。本文是在“镀与钍试剂Ⅰ的极谱研究”的基础上,用抗坏血酸消除铬酸根的干扰,用EDTA消除铁、铅、镉等干扰,并应用于矿石中微量铍的测定。本法基于铍在NH_4Cl-NH_4OH介质中与钍试剂Ⅰ生成络合物,在-0.55伏产生灵敏度较高的极谱波,可测到0.005微克/毫升的铍。本法具有干扰少,可直接测定矿石中微量铍。     

矿石中微量铍的极谱测定

铍的极谱测定研究不多,最近已有人报导了用铍试剂Ⅲ测定矿石中微量铍的催化极谱法。本文是在“铍与钍试剂Ⅰ的极谱研究”的基础上,用抗坏血酸消除铬酸根的干扰,用EDTA消除铁、铅、镉等干扰,并应用于矿石中微量铍的测定。本法基于铍在NH_4Cl-NH_4OH介质中与钍试剂Ⅰ生成络合物,在-0.55伏产生灵敏度较高的极谱波,可测到0.005微克/毫升的铍。本法具有干扰少,可直接测定矿石中微量铍。     

极谱络合吸附波测定微量硼的研究

用极谱法测定硼是比较困难的,多年来国内外在这方面报道很少。文献介绍有碘化四甲基铵法和甘露醇一亚硫酸钠法等,前者的E_(1/2)为-1.9伏;后者E_(1/2)-0.56和-1.04伏有两个波,用示波极谱可测定0.1微克/毫升,但在实际分析中均未得到推广和应用。本文受铍试剂Ⅲ分光光度法测定硼和示波极谱法测定铍的启发,研究了铍试剂Ⅲ极谱络合吸附波测定的体系并对其机理进行了初步的探讨,得出铍试剂Ⅲ与硼的络合物吸附在电极上,其中配位体铍试剂Ⅲ产生的还原波。方法具有较高的灵敏度,0.025—5微克/10毫升的硼与峰电流呈线性关系。能简便地测定岩石土壤中的微量硼并取得满意结果。     

催化反应—示波极谱法测定痕量碘

催化反应－示波极谱分析^[1-5]系催化动力学分析的一个有待进一步研究的领域，金属元素的催化反应一示波极谱法已有研究报道^[1-7]，但非金属元素（碘）的催化反应－示波极谱法还少见。     

Internally-Consistent Thermodynamic Data for Minerals in the System Na2O-K2O-CaO-MgO-FeO-Fe2O3-Al2O3-SiO2-TiO2-H2O-CO2

Internally consistent standard state thermodynamic data arepresented for 67 minerals in the system Na₂O-K₂O-CaO-MgO-FeO-Fe₂O₃-Al₂O₃-SiO₂-TiO₂-H₂O-CO₂.The method of mathematical programming was used to achieve consistencyof derived properties with phase equilibrium, calorimetric,and volumetric data, utilizing equations that account for thethermodynamic consequences of first and second order phase transitions,and temperature-dependent disorder. Tabulated properties arein good agreement with thermophysical data, as well as beingconsistent with the bulk of phase equilibrium data obtainedin solubility studies, weight change experiments, and reversalsinvolving both single and mixed volatile species. The reliabilityof the thermodynamic data set is documented by extensive comparisons(Figs. 4–45) between computed equilibria and phase equilibriumdata. The high degree of consistency obtained with these diverseexperimental data gives confidence that the refined thermodynamicproperties should allow accurate prediction of phase relationshipsamong stoichiometric minerals in complex chemical systems, andprovide a reasonable basis from which activity models for mineralsmay be derived.     

Siderit-Magnesit-Mischkristallbildung im system Mg2+-Fe2+-CO 3 2− -Cl 2 2− -H2O

The formation of the solid solution series MgCO₃-FeCO₃ in the system Mg²⁺-Fe²⁺-CO ₃ ^2? -Cl ₂ ^2? -H₂O has been investigstad between 200° C and 500° C. The experimental results show that the composition of any of these carbonates strongly depends on the temperature: At high temperatures mixed crystals rich in MgCO₃ are formed and low temperatures lead to the formation of FeCO₃-rich carbonates. Thus, at 200° C a Fe-poor (Mg-rich) solution is in equilibrium with a Fe-rich carbonate. At temperatures higher than 350° C a Fe-rich (Mg-poor) solution coexists with a Fe-poor (Mg-rich) solid phase; see Fig. 1. At 350° C a solution with a mole fraction^mFe²⁺/(^mFe²⁺+^mMg²⁺) of 0.20 leads to the formation of magnesite very poor in Fe, whereas at 250° C the same solution is in equilibrium with sideroplesit, containing 80 Mol-% FeCO₃, see Figs. 2 and 3. The importance of the experimental results for the formation of deposits of magnesite and siderite is discussed.     

Electrochemical Evidence for Pentasulfide Complexes with Mn2+, Fe2+, Co2+, Ni2+, Cu2+ and Zn2+

A series of stable pentasulfide complexes of the common base metals, Mn, Fe, Co, Ni, Cu and Zn exist in aqueous solutions at ambient temperatures. Pure sodium pentasulfide was prepared and reacted with the divalent cations of Mn, Fe, Co, Ni, Cu and Zn in aqueous solution at ambient temperature. The S52- complexes were found to exist as determined by voltammetric methods.Pentasulfide complexes with compositions assigned as [M(1-S5)] and [M2(- S5)]2+ occur for Mn, Fe, Co and Ni where only one terminal S atom in the S52- binds to one metal (1 = mono-dentate ligand or M-S-S-S-S-S, = ligand bridging two metal centers or M-S-S-S-S-S-M). Conditional stability constants are similar for all four metals with log 1 between 5.3 and 5.7 and log 2 between 11.0 and 11.6. The constants for these pentasulfide complexes are similar to the tetrasulfide complexes and are approximately 0.4–0.8 log units higher than for comparable bisulfide complexes [M(SH)]+ as expected based on the higher nucleophilicity of S52- compared to HS-. Voltammetric results indicate that these are labile complexes.As with the bisulfide and tetrasulfide complexes, Zn(II) and Cu(II) are chemically distinct from the other metals. Zn(II) reacts with pentasulfide to form a stable monomeric pentasulfide chelate, [Zn(1-S5)] with log = 8.7. Cu(II) reacts with pentasulfide to form a complex with the probable stoichiometry [Cu(S5)]2 with log estimated to be 20.2. As with the other four metals, these complexes are comparable with the tetrasulfide complexes. Discrete voltammetric peaks are observed for these complexes and indicate they are electrochemically inert to dissociation. Reactions of Zn(II) and Cu(II) also lead to significant breakup of the polysulfide.The relative strength of the complexes is Cu > Zn > Mn, Fe, Co, Ni. Cu displaces Zn from [Zn(1- S5)] and both Cu and Zn displace Mn, Fe, Co and Ni from their pentasulfide complexes.     

Single crystal raman studies of pyrite-type RuS2, RuSe2, OsS2, OsSe2, PtP2, and PtAs2

Single crystal Raman spectra of pyrite-type RuS₂, RuSe₂, OsS₂, OsSe₂, PtP₂, and PtAs₂ are presented and discussed with reference to the energies of the X-X stretching modes _x-x (A _g, F _g) and the X₂ librations (E, 2F_g). The main results obtained are (i) strong Raman resonance effects, (ii) different sequences for _x-x (A _g) and (E _g), i.e., R_{x_2 } $$ " align="middle" border="0"> for PtP₂ and PtAs₂ and R_{x_2 } $$ " align="middle" border="0"> for OsS₂, owing to the interplay of intraionic and interionic lattice forces, (iii) greater strengths for the intraionic P-P and As-As bonds compared to the S-S and Se-Se bonds, respectively, and (iv) a strong influe_gnce of the metal ions on the strength of the X-X bonds.This is contribution LXI of a series of papers on lattice vibration spectra     

Gehlenite stability in the system CaO-Al2O3-SiO2-H2O-CO2

P, T, \(X_{{\text{CO}}_{\text{2}} }\) relations of gehlenite, anorthite, grossularite, wollastonite, corundum and calcite have been determined experimentally at P _f =1 and 4 kb. Using synthetic starting minerals the following reactions have been demonstrated reversibly

1. 2 anorthite+3 calcite=gehlenite+grossularite+3 CO₂.
2. anorthite+corundum+3 calcite=2 gehlenite+3 CO₂.
3. 3anorthite+3 calcite=2 grossularite+corundum+3CO₂.
4. grossularite+2 corundum+3 calcite=3 gehlenite+3 CO₂.
5. anorthite+2 calcite=gehlenite+wollastonite+2CO₂.
6. anorthite+wollastonite+calcite=grossularite+CO₂.
7. grossularite+calcite=gehlenite+2 wollastonite+CO₂.

In the T, \(X_{{\text{CO}}_{\text{2}} }\) diagram at P _f =1 kb two isobaric invariant points have been located at 770±10°C, \(X_{{\text{CO}}_{\text{2}} }\) =0.27 and at 840±10°C, \(X_{{\text{CO}}_{\text{2}} }\) =0.55. Formation of gehlenite from low temperature assemblages according to (4) and (2) takes place at 1 kb and 715–855° C, \(X_{{\text{CO}}_{\text{2}} }\) =0.1–1.0. In agreement with experimental results the formation of gehlenite in natural metamorphic rocks is restricted to shallow, high temperature contact aureoles.     

Heat capacity of minerals in the system Na2O-K2O-CaO-MgO-FeO-Fe2O3-Al2O3-SiO2-TiO2-H2O-CO2: representation,estimation, and high temperature extrapolation

A revised equation is proposed to represent and extrapolate the heat capacity of minerals as a function of temperature: C _P=k₀+k₁ T ^–0.5+k₂ T ^–2+k₃ T ^–3 (where k₁, k₂0).This equation reproduces calorimetric data within the estimated precision of the measurements, and results in residuals for most minerals that are randomly distributed as a function of temperature. Regression residuals are generally slightly greater than those calculated with the five parameter equation proposed by Haas and Fisher (1976), but are significantly lower than those calculated with the three parameter equation of Maier and Kelley (1932).The revised equation ensures that heat capacity approaches the high temperature limit predicted by lattice vibrational theory (C _P=3R+²VT/). For 16 minerals for which and have been measured, the average C _Pat 3,000 K calculated with the theoretically derived equation ranges from 26.8±0.8 to 29.3±1.9 J/(afu·K) (afu = atoms per formula unit), depending on the assumed temperature dependence of . For 91 minerals for which calorimetric data above 400 K are available, the average C _Pat 3,000 K calculated with our equation is 28.3±2.0 J/(afu·K). This agreement suggests that heat capacity extrapolations should be reliable to considerably higher temperatures than those at which calorimetric data are available, so that thermodynamic calculations can be applied with confidence to a variety of high temperature petrologic problems.Available calorimetric data above 250 K are fit with the revised equation, and derived coefficients are presented for 99 minerals of geologic interest. The heat capacity of other minerals can be estimated (generally within 2%) by summation of tabulated oxide component C _Pcoefficients which were obtained by least squares regression of this data base.     

Studies in the system KAlSiO4-BaAl2Si2O8-SiO2-H2O

Various members of the KAlSi₃O₈-BaAl₂Si₂O₈ feldspar series are hydrothermally synthesized. Cellparameters of these are calculated from diffractometer patterns and found to be similar to those of Gay and Roy. A variation diagram is constructed correlating Cn-content and values of Δ_FeKα(2θ₍₁₁₁₎CaF₂—2θ₍₀₀₄₎Fs_ss), which gives $${\text{Mol}}\% {\text{ Cn = 229}}{\text{.83}}\Delta {\text{2}}\theta ---{\text{190}}{\text{.81}}$$ by a least square regression fitting. Phase equilibria relation in the solidus-liquidus-region for the KAlSi₃O₈-BaAl₂Si₂O₈-H₂O system at 1000 kg/cm² are investigated. It is found to be a case of simple solid solution in a binary system, with reservations at the potassium-rich side of the system. Goranson (1938) gives a temperature of about 1000°C at 1000 kg/cm² \(P_{{\text{H}}_{\text{2}} {\text{O}}} \) for the incongruent melting of sanidine, but the authors prefer a value around 930°C at the same \(P_{{\text{H}}_{\text{2}} {\text{O}}} \) . Reaction products of starting materials on the join KAlSi₂O₆-BaAl₂Si₂O₈ and KAlSiO₄-BaAl₂Si₂O₈ gave no experimental hint for replacement of K⁺ by Ba⁺⁺.