Solubility in the system sodium orthophosphate, acetone, and water

Nirenberg, Zvi; Solenchyk, Beatrice; Yaron, I.

doi:10.1021/je60072a003

Cited by 4 publications

(3 citation statements)

References 0 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…The removal of phosphates was not tested, because trisodium phosphate (Na 3 PO 4 ) is the only phosphate that is soluble in water, but it is insoluble in an aqueous solution of 60 vol % acetone. [23] We conclude that the total of non-nitrate oxygen derived from the sample and laboratory material is ≤2 mmol. isotopic measurements of the blank from the Miramichi water and VALSER W water (contribution of 2.7% and 2.6%) we estimate that the lower boundary is more reasonable.…”

Section: Removal Of Interfering Compoundsmentioning

confidence: 74%

“…Furthermore, no sulfate and only small amounts of chloride were found. The removal of phosphates was not tested, because trisodium phosphate (Na 3 PO 4 ) is the only phosphate that is soluble in water, but it is insoluble in an aqueous solution of 60 vol % acetone . We conclude that the total of non‐nitrate oxygen derived from the sample and laboratory material is ≤2 µmol.…”

Section: Resultsmentioning

confidence: 99%

“…The freeze-dried salts are first suspended in 350 mL 1 M NaI solution (sodium iodide, 99.999% trace metal basis; Aldrich, Munich, Germany) with a vortex shaker for 1-2 min, and [26],b na na CaSO 4 20 0.298 [26] na na Na 3 PO 4 *12H 2 O 20 10.8 [26] 20 0.17 [23],d Ba(NO 3 ) 2 20 8.27 [26] 25 0.0002 [27] K 2 SO 4 20 10.0 [26] 25 0.03 [26],e Na 2 SO 4 20 16.3 [26] 33 0.44 [28],f Na 2 CO 3 20 18.0 [26] 35 0.02 [28],g KNO 3 20 24.0 [26] 25 0.015 [27] MgSO 4 *7H 2 O 20 25.2 [26] na na KCl 20 25.4 [26] 25 0.00091 [29],c BaCl 2 *2H 2 O 20 26.3 [26] na insoluble [30] NaCl 20 26.37 [26] 25 0.00042 [29],c MgCl 2 *6H 2 O 20 35.3 [26] 25 0.0031 [31] Mg(NO 3 ) 2 *6H 2 O 25 42.1 [26] na very soluble [32] CaCl 2 *6H 2 O 20 42.7 [26] 20 0.0101 [26],c NaNO 3 20 46.7 [26] 25 0.024 [27]…”

Section: Experimental Nitrate Isolation Proceduresmentioning

confidence: 99%

See 2 more Smart Citations

A new isolation procedure of nitrate from freshwater for nitrogen and oxygen isotope analysis

Huber

Bernasconi

Luster

et al. 2011

Rapid Comm Mass Spectrometry

View full text Add to dashboard Cite

The nitrogen (δ(15)N) and oxygen isotope (δ(18)O) analysis of nitrate (NO(3)(-)) from aqueous samples can be used to determine nitrate sources and to study N transformation processes. For these purposes, several methods have been developed; however, none of them allows an accurate, fast and inexpensive analysis. Here, we present a new simple method for the isolation of nitrate, which is based on the different solubilities of inorganic salts in an acetone/hexane/water mixture. In this solvent, all major nitrate salts are soluble, whereas all other oxygen-bearing compounds such as most inorganic carbonates, sulfates, and phosphates are not. Nitrate is first concentrated by freeze-drying, dissolved in the ternary solvent and separated from insoluble compounds by centrifugation. Anhydrous barium nitrate is then precipitated in the supernatant solution by adding barium iodide. For δ(18)O analysis, dried Ba(NO(3))(2) samples are directly reduced in a high-temperature conversion system to CO and measured on-line using isotope ratio mass spectrometry (IRMS). For δ(15)N analysis, samples are combusted in an elemental analyzer (EA) coupled to an IRMS system. The method has been tested down to 20 µmol NO(3)(-) with a reproducibility (1SD) of 0.1‰ for nitrogen and 0.2-0.4‰ for oxygen isotopes. For nitrogen we observed a small consistent (15) N enrichment of +0.2‰, probably due to an incomplete precipitation process and, for oxygen, a correction for the incorporation of water in the precipitated Ba(NO(3))(2) has to be applied. Apart from being robust, this method is highly efficient and low in cost.

show abstract

Section: Removal Of Interfering Compoundsmentioning

confidence: 74%

Section: Resultsmentioning

confidence: 99%

Section: Experimental Nitrate Isolation Proceduresmentioning

confidence: 99%

See 1 more Smart Citation

A new isolation procedure of nitrate from freshwater for nitrogen and oxygen isotope analysis

Huber

Bernasconi

Luster

et al. 2011

Rapid Comm Mass Spectrometry

View full text Add to dashboard Cite

show abstract

Trisodium Phosphate

Eysseltová

1988

Alkali Metal Orthophosphates

View full text Add to dashboard Cite

1) Trisodium phosphate; Na3P04 ; J. Eysseltova" [7601-54-9] Charles University (2) Water; H^O; [7732-18-5] Prague, Czechoslovakia May 1985 CRITICAL EVALUATION: THE BINARY SYSTEMThere is a good deal of uncertainty about this system. There is disagreement about the solubility and about the composition of the solid phase. The data published by Apfel (1) for the solubility of trisodium phosphate over the temperature range of 273-356 Κ disagree with the data of Mulder (2) as quoted by others (3). Kobe and Leipper (4) reported the solubility of a substance having the composition Na3P04*l/7NaOH # 12H20 and their results agree to some extent with those of Apfel (1). Ravich and Shcherbakova (5) reported the existence of solid solutions mNa3P04·ηΝ3Η2Ρ04 in equilibrium with saturated solutions having Na/P ratios = 1/3 above 523 K.The matter of the hydrates of Na^PO^ has also been the subject of disagreement. Most authors consider Na3P04*12H20 to be the solid phase at temperatures below 323 K, but Wendrow and Kobe (3) suggest that it is Na3P04*l/4NaOH-12H20. The solid phase in equilibrium with saturated solutions is reported to be Na3PO4*10H2O over the temperature range 323-333 Κ and Na3P04'8H20 at temperatures from 343 to 348 Κ (1). But others (3), on the basis of extrapolated data, suggest that the equilibrium solid phases are Na3P04'l/4NaOH"12H20 at temperatures up to 328 K, Na3P04*8H20 from 328-338 K, and Na3P04*6H20 from 338-373 K. More work is needed to clarify the nature of the solid phases before the solubility data can be evaluated.Schroeder, et al. (6) made solubility measurements over the temperature interval 348-523 K. They reported the equilibrium solid phase to be Na3P04*H20 in the temperature interval 393-488 Κ and the anhydrous Na3P04 to be the solid phase above 488 K. Attempts to fit these data to the general solubility equations described and discussed in the section on NaH2P04 (chap. 3) were unsuccessful. The number of experimental points re maining after the iteration was too small to consider the results to be reasonable. Perhaps a different model is needed to treat these data. MULTICOMPONENT SYSTEMSThe phase diagrams for systems in which Na^PO^ is a component differ substantially from those in which NaH2P04 or Na2HP04 are components. The latter usually form simple eutonic systems, while with systems containing Na3P04 the formation of solid solutions or complex compounds has often been reported.Solubility values reported for these systems often disagree with each other. This is probably due to the chemical complexity of the systems and the fact that the analyses are complicated by the high pH values of these systems.No solid solutions or complex compounds have been reported as equilibrium solid phases for the following systems: Na3P04-NaN02-H20 at 298 Κ (7); Na3P04-NaCl-H20 at 298 and 378 Κ (8); Na^O^N^WO^O at 503 Κ (9); Na3P04-Na2C03-H20 at 273 and 293 Κ (10), and 298 Κ (11).The presence of a small amount of NaOH in one study of the last system above (4) resulted in only a small increase in the concentr...

show abstract

Isobaric Vapor−Liquid Equilibrium of Binary Mixtures of 1-Butanol + Chlorobenzene and 2-Butanol + Chlorobenzene at 20 and 100 kPa

et al. 1997

View full text Add to dashboard Cite

Isobaric vapor-liquid equilibria were obtained for 1-butanol + chlorobenzene and for 2-butanol + chlorobenzene systems at 20 and 100 kPa using a dynamic still. The experimental error in temperature was (0.1 K, in pressure (0.01 kPa and (0.1 kPa for the experiments carried out at 20 and 100 kPa, respectively, and in liquid and vapor composition (0.001. The two systems satisfy the point-to-point thermodynamic consistency test. Both systems show a positive deviation from ideality. The data were correlated with the Wilson equation.

show abstract

Solubility in the system sodium orthophosphate, acetone, and water

Cited by 4 publications

References 0 publications

A new isolation procedure of nitrate from freshwater for nitrogen and oxygen isotope analysis

A new isolation procedure of nitrate from freshwater for nitrogen and oxygen isotope analysis

Trisodium Phosphate

Isobaric Vapor−Liquid Equilibrium of Binary Mixtures of 1-Butanol + Chlorobenzene and 2-Butanol + Chlorobenzene at 20 and 100 kPa

Contact Info

Product

Resources

About