Studies on the Hydrolysis of Metal Ions. 21. The Hydrolysis of the Tin(II) Ion, Sn2+.

Tobias, R. Stuart; Rydberg, Jan; Stenhagen, Einar; Zackrisson, Margareta; Ernster, Lars; Diczfalusy, E.

doi:10.3891/acta.chem.scand.12-0198

Cited by 79 publications

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“…I t had been previously noted that the dimethyltin(1V) ion behaved, qualitatively, much like the tin(1I) ion (8); and it had been shown some time ago that polynuclear hydrolysis products exist in hydrolyzed tin(I1) solutions (9). Indeed, it was found that in addition to the simple conjugate base (CH3) 2SnOH+ appreciable concentrations of a binuclear species ((CH3) zSn (OH)) 2+2 were formed in the hydrolyzed dimethyltin perchlorate solutions.…”

Section: '782mentioning

confidence: 99%

Studies on the Soluble Intermediates in the Hydrolysis of Dimethyltin Dichloride: Equilibrium Constant Fitting With a High Speed Digital Computer

Tobias¹,

Yasuda²

1964

Can. J. Chem.

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The hydrolysis of (CH3)2SnC12 has been studied in a medium 0.1 M in (Naf)C1-by a potentiometric titration technique. The complexes formed by the hydrolysis reactions together with their formation constants have been determined by analysis of the 394 data sets using a high speed digital computer. The data can be fitted equally well over the range pH 1.5 to 9 by the four formation constants for (CH3)2SnOH+ (log *Pi1 = -3.245+0.004), [(CH3)2-SIIOH]~'~ (log *Pzz = -5.00Zk0.02), (CH~)~SXI(OH)~ (log * P z~ = -8.5162~ 0.004), and [(CH3)2-Sn]a(OH2ef2 (log *Ps4 = -16.85zk0.02) or by the five constants for (CH3)2SnOH+ (log *PI,(log *P22 = --5.05+0.02), (CH3)2Sn(OH), (log *Pzl = -8.5351 0.005), ((CH3)2Sn)2(OH)3: (log *Pa2 = r9.81rt0.01), and ((CH3)2Sn)3(OH) 4+2 (log *Pa3 = -11.52~t0.03). Thus there is little question about the existence in the solutions of the simple monohydroxo complex and its diiner or of the neutral dihydroxide. Only very low concentrations of species containing more than four tin atoms can exist in aqueous solution. I n addition, the data determined previously for the hydrolysis of (CH3)2Sn(C104)2 in a tnediuin 3.0 M in (Na+)C104-have been refined by the least squares procedure. These 762 data sets can also be fitted equally well by the set of constants log *fi,, = -3.554~0.01, log *Pzz = -4.52 10.01, log *&I = -9.00rt0.01, and log * P G~ = -16.14rt0.03 or log *PI, = -3.54Zk0.01, log *Pzz = -4.60Zk0.02, log *@,I = -8.98f 0.01, log *P32 = -9.7610.06, and log *P43 = -10.404~ 0.05. The tendency of dimethyltin dichloride to form polycondensed species in aqueous solution is slight, and there is no evidence for the formation of large rings or chains. The solid stannoxane which precipitates from chloride solution was studied by infrared and X-ray powder photography and is essentially the same as the con~pound obtained by reaction of (CH3)2Sn0 and (CH3)2SnC12 in a 1:l mole ratio in 95% ethanol. This corresponds to a slightly different product than that obtained by a 1:1 reaction of these compounds in benzene which gives ((CH3)2SnCl)20. This is in accord with the observation that precipitation occurs only a t a pH higher than that a t which ( ( C H~)~S~O H ) Q +~ has attained the maximum concentration, and hence precipitation is occasioned by the formation of larger polycondensed species. A comparison of the perchlorate and chloride data also indicatesthat the tendency to form polycondeilsed species is reduced by the presence of-chloride ion. This is partially an ionic strength effect and partially a result of chloride coinplexi~lg of the simple aquodimethyltin(1V) ion, and the first chloro-complexing constant was mtimated to be 28 I, mole-'. INTRODUCTIOS

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Section: '782mentioning

confidence: 99%

Studies on the Soluble Intermediates in the Hydrolysis of Dimethyltin Dichloride: Equilibrium Constant Fitting With a High Speed Digital Computer

Tobias¹,

Yasuda²

1964

Can. J. Chem.

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“…2.20 [Bates and Acree, 1943); HF, pK 3.45 [Weast, 1976]; SnOH*, pK 3.9 [Tobias, 1958]; S n,(O H );\ pK 4.4 [ Tobias, 1958]; S n,(O H );\ pK 6.8 [Tobias, 1958]; SnF*, pK -4.8 [Connick and Paul, 1961]; SnFj, pK -9.9 [Schaap et al, 1954].…”

Section: Preparation and Measurement O F Solutionsmentioning

confidence: 99%

On the Properties of Fluoride Solutions Used for Topical Treatment and Mouth Rinse

Larsen¹,

Jensen²

1986

Caries Res

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A number of solutions used for topical application and mouth rinsing were analyzed and calcium fluoride formation on human enamel at 20 °C determined. In most solutions free fluoride and hydrogen fluoride were the main ion species, whereas stannous hydroxide and stannous fluoride ion pairs were the dominating components of stannous fluoride solutions. The calcium fluoride formation on enamel was assessed by chemical analysis. It was found that an increase in fluoride activity and a decrease in pH increased the calcium fluoride formation to almost the same extent.

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“…A number of repeat experiments were carried out with initial tin(II) sulphate concentrations ranging between 0.03 and 0.06 M and equilibrated in a thermostatted water bath at 25~ Reaction vessels were wrapped in aluminium foil to exclude light, thought to promote the oxidation of tin(II) under certain conditions (Tobias, 1958).…”

Section: Methodsmentioning

confidence: 99%

“…Tin activity was measured using a tin amalgam electrode and a saturated calomel reference electrode. This was calibrated with tin(II) perchlorate following the method of Tobias (1958). The ionic strengths of the solutions were brought to 1 M by adding NaC104(s).…”

Section: Sn30(oh)2so 4 Solutionsmentioning

confidence: 99%

The stabilities of secondary tin minerals. Part 2: The hydrolysis of tin(II) sulphate and the stability of Sn₃O(OH)₂SO₄

1996

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Tritin(II)dihydroxyoxosulphate, Sn30(OH)2SO4, is a rare corrosion product found on the surfaces of certain tin alloys. A new synthesis based on the hydrolysis of SnSO4 is described. The stability constant determination of Sn30(OH)2SO4,s, at 298.2K and 105pa is determined using direct measurements via electrodes, of the activities of tin(II) and sulphate ions. AfG~ is equal to -1563.1 ___ 0.9 kJ mo1-1.

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Studies on the Hydrolysis of Metal Ions. 21. The Hydrolysis of the Tin(II) Ion, Sn2+.

Cited by 79 publications

References 0 publications

Studies on the Soluble Intermediates in the Hydrolysis of Dimethyltin Dichloride: Equilibrium Constant Fitting With a High Speed Digital Computer

Studies on the Soluble Intermediates in the Hydrolysis of Dimethyltin Dichloride: Equilibrium Constant Fitting With a High Speed Digital Computer

On the Properties of Fluoride Solutions Used for Topical Treatment and Mouth Rinse

The stabilities of secondary tin minerals. Part 2: The hydrolysis of tin(II) sulphate and the stability of Sn₃O(OH)₂SO₄

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Studies on the Hydrolysis of Metal Ions. 21. The Hydrolysis of the Tin(II) Ion, Sn2+.

Cited by 79 publications

References 0 publications

Studies on the Soluble Intermediates in the Hydrolysis of Dimethyltin Dichloride: Equilibrium Constant Fitting With a High Speed Digital Computer

Studies on the Soluble Intermediates in the Hydrolysis of Dimethyltin Dichloride: Equilibrium Constant Fitting With a High Speed Digital Computer

On the Properties of Fluoride Solutions Used for Topical Treatment and Mouth Rinse

The stabilities of secondary tin minerals. Part 2: The hydrolysis of tin(II) sulphate and the stability of Sn3O(OH)2SO4

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The stabilities of secondary tin minerals. Part 2: The hydrolysis of tin(II) sulphate and the stability of Sn₃O(OH)₂SO₄