Potentiometric Determination of the Solubility Product of Lead Carbonate.

Näsänen, Reino; Meriläinen, Paavo; Leppänen, Kaarina

doi:10.3891/acta.chem.scand.15-0913

Cited by 19 publications

(11 citation statements)

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“…This, together with the veI)' low solubility prochict of PbC03 (K,p = 10-1 3 1 3 at 25C; Nasanen et al, 1961), results in a sharp increase of the supersaturation of the solution with respect to cemssite. As a result, some time after the phosgenite has been dissolving, the critical supersaturation foc cemssite is reached for cerussite crystals nucleating on the (001) phosgen ite smface.…”

Section: Evolution Of Supersaturation During the Dissolution-precipitmentioning

confidence: 99%

In situ atomic force microscope observations of a dissolution–crystallisation reaction: the phosgenite–cerussite transformation

Pina

Fernández-Dı́az

Prieto

et al. 2000

Geochimica et Cosmochimica Acta

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Abstract-The dissolution-reprecipitation reaction of phosgenite (Pb2CI2C03) to cerussite (PbC03) has been observed in situ in a fluid cell of an atomic force microscope (AFM). The (00 I) face of phosgenite, in contact with static carbonated aqueous solutions, rapidly begins to dissolve. AFM observations show that dissolution occurs by generation and spread of square-shaped etch pits with sides parallel to (I 10) directions. The dissolution of the (110) steps is isotropic and the etch pits therefore remain square shaped during the dissolution process, as dictated by the existence of a fourfold axis perpendicular to the phosgenite (00 I) face. Two types of (110) etch pits were found: short-lived shallow pits, of one unit cell depth (8.8 A), and deep pits, which rapidly reach depths between 10 and 60 nrn. A few minutes after the dissolution begins, only the deep pits remain and subsequent dissolution of the phosgenite (001) surface proceeds by increasing their width and depth. The increase of Pb 2 + and CO�-concentration in the aqueous solution as a consequence of the dissolution sharply increases the supersaturation for PbC03. As a result, after a certain incubation time, cerussite crystals nucleate on the phosgenite (001) surface and a coupled process of dissolution-crystallisation starts. Cerussite crystals, which grow by a spiral-growth mechanism, distort the concentration field around them. As a consequence, phosgenite dissolution is accelerated in the proximity of such growing cerussite individuals and both the fonnation of new deep etch pits and the development of irregular dissolution fronts are observed. Further phosgenite dissolution leads to an increase of cerussite nucleation and growth rates, in such a way that this dissolution-crystallisation phenomenon can be considered as an autocatalytic process.

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Section: Evolution Of Supersaturation During the Dissolution-precipitmentioning

confidence: 99%

In situ atomic force microscope observations of a dissolution–crystallisation reaction: the phosgenite–cerussite transformation

Pina

Fernández-Dı́az

Prieto

et al. 2000

Geochimica et Cosmochimica Acta

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“…Na 2 CO 3 are considered as the equilibrium values, and are used in the following modeling. It is assumed that steady-state concentrations represent equilibrium concentrations, as the duration of experiments in this work, up to 1461 days, is significantly longer than previous studies such as those of Nasanen et al [6], and Bilinski and Schindler [7] under similar conditions. For instance, the experiments of Nasanen et al [6] lasted only for up to 52 h (i.e., 2.2 days).…”

Section: Resultsmentioning

confidence: 99%

“…The log K s o [-13.76 ± 0.15 (2r), and the uncertainty referring to 2r hereafter in the text] determined in this study is slightly lower than the value of -13.13 at infinite dilution determined by Nasanen et al [6]. Bilinski determined the equilibrium quotient (log Q) at 0.3 mol dm -3 (0.305 mol kg -1 ) for the following reaction:…”

Section: The Formation Reaction For Pbco 3 (Aq) Is Written Asmentioning

confidence: 90%

Experimental determination of lead carbonate solubility at high ionic strengths: a Pitzer model description

Xiong

2015

Monatsh Chem

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In this study, solubility measurements of lead carbonate, PbCO 3 (cr), cerussite, as a function of total ionic strengths are conducted in the mixtures of NaCl and NaHCO 3 up to I = 1.2 mol kg -1 and in the mixtures of NaHCO 3 and Na 2 CO 3 up to I = 5.2 mol kg -1 , at room temperature (22.5 ± 0.5°C). The solubility constant (log K s o ) for cerussite was determined as -13.76 ± 0.15 (2r) with a set of Pitzer parameters describing the specific interactions of PbCO 3 (aq), Pb CO 3 ð Þ 2À 2 , and Pb(CO 3 )Cl -with the bulk-supporting electrolytes, based on the Pitzer model. The model developed in this work can reproduce the experimental results including model-independent solubility values from the literature over a wide range of ionic strengths with satisfactory accuracy. The model is expected to find applications in numerous fields, including the accurate description of chemical behavior of lead in geological repositories, the modeling of formation of oxidized Pb-Zn ore deposits, and the environmental remediation of lead contamination. Graphical abstract 1.0E-06 1.0E-05 1.0E-04 1.0E-03 1.0E-02 0 1 2 3 4 5 6 m[Pb(II)tot]/mol•kg -1 0.046 mol kg ¹ NaHCO + 0.054 mol kg ¹ Na CO 0.11 mol kg ¹ NaHCO + 0.19 mol kg ¹ Na CO 0.26 mol kg ¹ NaHCO + 0.54 mol kg ¹ Na CO 0.33 mol kg ¹ NaHCO + 0.87 mol kg ¹ Na CO 0.40 mol kg ¹ NaHCO + 1.4 mol kg ¹ Na CO 0.42 mol kg ¹ NaHCO + 1.58 mol kg ¹ Na CO Model developed in this study, theta parameters = 0 Model developed in this study, theta parameters 0 Total ionic strength/mol•kg -1

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“…Some of them were calculated from activity data for single electrolytes [12][13][14] and from potentiometric [4,5,21,[26][27][28][29][30][31][32] and solubility [15][16][17][18][33][34][35][36][37][38][39][40][41][42][43][44][45][46][47][48][49] studies. Uncertainty is conditioned mainly by insignificant variation of the parameter b ij with ionic strength and, in the majority of cases, specifies applicability of the model to the description of experimental data.…”

Section: Major Componentsmentioning

confidence: 99%

“…The values b(CO 2(aq) , j ) and formation constant for HCO + 2 complex were calculated from the solubility of carbon dioxide in salt solutions (Fig. 1) [26], NaCl [27], KCl and NaClO 4 [28] solutions. Right upper panel: second dissociation constant of sulfuric acid in NaCl [29] and NaClO 4 (hollow circles: [30]; box: [31]) solutions.…”

Section: Major Componentsmentioning

confidence: 99%

Modeling of ionic equilibria of trace metals (Cu2+, Zn2+, Cd2+) in concentrated aqueous electrolyte solutions at 25 °C

Pivovarov

2005

Journal of Colloid and Interface Science

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Potentiometric Determination of the Solubility Product of Lead Carbonate.

Cited by 19 publications

References 0 publications

In situ atomic force microscope observations of a dissolution–crystallisation reaction: the phosgenite–cerussite transformation

In situ atomic force microscope observations of a dissolution–crystallisation reaction: the phosgenite–cerussite transformation

Experimental determination of lead carbonate solubility at high ionic strengths: a Pitzer model description

Modeling of ionic equilibria of trace metals (Cu2+, Zn2+, Cd2+) in concentrated aqueous electrolyte solutions at 25 °C

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