Polarographic analysis of lead(IV) species in solutions containing sulfuric and phosphoric acids

Amlie, R. F.; Berger, Terry A.

doi:10.1016/s0022-0728(72)80264-x

Cited by 15 publications

(12 citation statements)

References 8 publications

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“…A second effect of phosphate is to solubilize lead(IV) as a phosphate species. Such species have been reported in phosphoric acid and mixed sulfuric-phosphoric acids (35)(36)(37). Compounds of lead(IV) and phosphate have been isolated (26, 35) with Pb:P ratios ranging from 1:1 to 1:6.…”

Section: Resultsmentioning

confidence: 97%

Cathodic stripping coulometry of lead

Laitinen¹,

Watkins²

1975

Anal. Chem.

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Section: Resultsmentioning

confidence: 97%

Cathodic stripping coulometry of lead

Laitinen¹,

Watkins²

1975

Anal. Chem.

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“…Pb(IV) complexes containing high phosphate concentrations have been produced chemically and electrochemically (Laitinen & Watkins, 1975;Huber & El-Meligy, 1969;Fleischmann et al, 1967;Bode & Voss, 1962). Using polarographic techniques, Amlie and Berger (1972) detected soluble Pb(IV) species in sulfuric acid only when phosphoric acid was present. However, no stability constants (or Gibbs free energies) and very few data exist for tetravalent lead hydroxide species, specifically tetravalent lead carbonate and phosphate complexes.…”

Section: -Bicarbonate Ion P-pressure Pb-lead Pbo 2 (S)-lead(iv) Oxmentioning

confidence: 99%

Formation of Pb(IV) oxides in chlorinated water

Lytle¹,

Schock²

2005

Journal AWWA

128

175

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Recent research has shown that Pb(IV) oxides play a significant geochemical role in drinking water distribution systems. However, most of the guidance for lead control in drinking water is based on the presumption that Pb(II) solids control lead solubility. Therefore, a better understanding of the chemistry of Pb(IV) in water is needed. Long‐term lead precipitation experiments were conducted in chlorinated water (1–3 mg/L Cl2) at pH 6.5, 8, and 10, with and without sulfate. Results showed that two Pb(IV) dioxide polymorphs—plattnerite (β‐PbO2) and scrutinyite (α‐PbO2)—formed over time, as long as a high suspension redox potential was maintained with free chlorine. Neither mineral formed spontaneously, and the rate of formation increased with increasing pH. Hydrocerrusite and/or cerrusite initially precipitated out and over time either disappeared or coexisted with PbO2. Water pH dictated mineralogical presence. High pH favored hydrocerrusite and scrutinyite; low pH favored cerrusite and plattnerite. Along with a transformation of Pb(II) to Pb(IV) came a change in particle color from white to a dark shade of red to dark grey (differing with pH) and a decrease in lead solubility. If free chlorine was permitted to dissipate, the aging processes (i.e., mineralogy, color, and solubility) were reversible.

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“…PbHPO, + 2H + = Pb +2 + H3PO4 [6] log aPb+-" = -1.8 --2 pH -log aH3PO ~ PbHPO~ + 2H~O = HPbO~-+ HPOc ~" + 3H + [7] log am,~o 2-= -39.1 + 3 pH -log a~l.o~ -2…”

Section: [3]mentioning

confidence: 99%

“…Several authors (4)(5)(6) have formed these complexes both chemically and electrochemically, but such complexes apparently occur only at HsPO4 concentrations above about 0.8% (10 g/l) in 35% H2SO4 (6). Several authors (4)(5)(6) have formed these complexes both chemically and electrochemically, but such complexes apparently occur only at HsPO4 concentrations above about 0.8% (10 g/l) in 35% H2SO4 (6).…”

mentioning

confidence: 99%

The Effect of Phosphoric Acid on the Positive Electrode in the Lead‐Acid Battery: III . Mechanism

Bullock

1979

J. Electrochem. Soc.

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Phosphoric acid added to battery electrolyte modifies the morphology of PbO2 corrosion films by reacting to produce Pbs(PO4)2 as an intermediate in the oxidation of Pb to PbO2. Because these modified PbO2 films resist reduction to PbSO4, battery failure from formation of a resistive PbSO4 film at the positive grid/active material interface is forestalled. Three new findings support this mechanism: (i) the identification of Pba(PO4)2 in lead corrosion films, (ii) the predictions of a thermodynamic model of the Pb/H2SO4/ H3PO4/H~O system, and (ii{) the measurement of sulfation rates of PbO2 films formed from Pba (PO4)2 and PbHPO4. * Electrochemical Society Active Member. ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 129.11.21.2 Downloaded on 2014-11-01 to IP Vol. I26, No. 11 LEAD-ACID BATTERY 1849 ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 129.11.21.2 Downloaded on 2014-11-01 to IP * Electrochemical Society Active Member.

show abstract

Polarographic analysis of lead(IV) species in solutions containing sulfuric and phosphoric acids

Cited by 15 publications

References 8 publications

Cathodic stripping coulometry of lead

Cathodic stripping coulometry of lead

Formation of Pb(IV) oxides in chlorinated water

The Effect of Phosphoric Acid on the Positive Electrode in the Lead‐Acid Battery: III . Mechanism

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