1313-82-2

Basic information

• Product Name: Sodium sulfide
• Synonyms: sodiumsulfide(anhydrous);sodiumsulfide(na2s);sodiumsulfide(non-specificname);sodiumsulfide,anhydrous;sodiumsulfide,hydrated,withnotlessthan30%water;sodiumsulfide[na2s];sodiumsulfuret;sodiumsulphide,anhydrous
• CAS NO: 1313-82-2
• Molecular Formula: Na2S
• Molecular Weight: 78.04
• EINECS: 215-212-0
• Product Categories: Inorganics;Inorganic Chemicals;Catalysis and Inorganic Chemistry;ChalcogenidesChemical Synthesis;Materials Science;Metal and Ceramic Science;metal chalcogenides;inorganic chemical raw material;inorganic salt;sulfate;sulfide
• Mol File: 1313-82-2.mol
• Article Data: 38

Chemical Properties

• Melting Point: 950 °C(lit.)
• Boiling Point: 174oC
• Appearance: Yellow/flakes
• Density: 1.86 g/mL at 25 °C(lit.)
• Storage Temp.: Refrigerator (+4°C)
• Solubility: H2O: 0.1 g/mL, clear, colorless
• Water Solubility: 186 g/L (20 ºC)
• Sensitive: Hygroscopic
• Stability: Spontaneously flammable. Incompatible with acids, metals, oxidizing agents. Contact with acid liberates toxic gas. Fine dust/air
• Merck: 14,8681
• CAS DataBase Reference: Sodium sulfide(CAS DataBase Reference)
• NIST Chemistry Reference: Sodium sulfide(1313-82-2)
• EPA Substance Registry System: Sodium sulfide(1313-82-2)

Safety Data

• Hazard Codes: C,N,Xn
• Statements: 31-34-50-22
• Safety Statements: 26-45-61-36/37/39
• RIDADR: UN 1849 8/PG 2
• WGK Germany: 2
• RTECS: WE1905000
• F: 3-8-9-23
• TSCA: Yes
• HazardClass: 4.2
• PackingGroup: II
• Hazardous Substances Data: 1313-82-2(Hazardous Substances Data)

Usage

Description

Sodium sulfide, also known as sodium sulfuret, is a water-soluble, yellowish to reddish, deliquescent powder with a strong alkaline reaction when dissolved in water. It has an odor of rotten eggs due to the emission of hydrogen sulfide when exposed to moist air. Sodium sulfide is a corrosive and readily oxidized material with variable composition, often containing polysulfides. It is used in various industries due to its reducing properties and as a chemical intermediate and solvent.

Uses

Used in Dye Industry:
Sodium sulfide is used as a raw material for the production of sulfur dyes, specifically sulfur green and sulfur blue. It is also used as a facilitator agent for dissolving sulfur dyes in the printing and dyeing industry.
Used in Paper Industry:
In the paper industry, sodium sulfide is used as a cooking agent in the production of high-grade paper. It is also used as a depressant and for collector desorption in non-metallic flotation.
Used in Tanning Industry:
Sodium sulfide is used for the hydrolysis of hair removal of raw skin and for the preparation of sodium polysulfide to help accelerate soaking and softening of dry skin.
Used in Fiber Textile Industry:
In the fiber textile industry, sodium sulfide is used for the denitrofication of artificial fiber textile, the reduction of nitration, and as a mordant for cotton fabric dyeing.
Used in Pharmaceutical Industry:
Sodium sulfide is mainly used for the production of antipyretic drugs such as phenacetin.
Used in Chemical Industry:
Sodium sulfide is used for making sodium thiosulfate, sodium hydrosulfide, and sodium polysulfide. It is also used as an analysis reagent and leather depilatory.
Used in Metallurgy:
Sodium sulfide is used in the oxidation process of gold, lead, and copper metal ores.
Used in Agriculture:
Sodium sulfide is used as a sheep dip.
Used in Miscellaneous Applications:
Sodium sulfide is used for H2S therapy to study its effect on the prevention of diabetes in animals. It is also used as a depilatory for leather, digestion auxiliary in paper-making, and in the textile, pigment, and rubber industries.
Industrial Uses:
Sodium sulfide is used as a depressant for quartz in the iron-activated and non-activated quartz flotation process. It is also used in the flotation of monazite, pyrochlore, zircon, and microcline, acting as a depressant and for the desorption of fatty acids.

Sodium sulfide

Sodium sulfide is also known as smelly soda and stinky base. At room temperature, the pure product is colorless or slightly purple prismatic crystal. The industrial sodium sulfide often exhibits pink, reddish brown or yellowish brown color for containing impurities. It has rotten egg smell and is corrosive and toxic. Its density is 2.427. It will be subject to decomposition at 920 ℃. It is soluble in cool water and easily soluble in hot water with dissolving in water almost fully being hydrolyzed into sodium hydroxide and sodium hydrosulfide (at 10 ℃, the solubility is 15.4; while the solubility is 57.2 g at 90 ℃). The aqueous water exhibits strongly alkalinity and is corrosive on copper, wood, skin, etc. It is slightly soluble in ethanol but insoluble in ether. When being encountered strong acid, the sodium sulfide will release hydrogen sulfide. It will be subject to deliquescence in air and is easily oxidized into sodium thiosulfate. Sodium sulfide is mainly used as the raw materials of hides depilatories, pulp cooking agent, and sulfur dye, the reducing agents of dye intermediates, fabric dyeing mordant, and ore flotation agent. It can also be used as viscose fiber desulfurizer and the raw material for production of sodium hydrosulfide and sodium polysulfide. The sodium sulfide in our county was originated in the 1830s. The production of it was earliest started from a chemical plant in Dalian, Liaoning in small-scale. Upon entering into the mid-1980s to the 1990s, with the vigorous development of the international chemical industry, the domestic industry had undergone a fundamental transformation with both the number and scale of production being dramatically increased with rapid development. The production area of sodium sulfide centered in Shanxi Yuncheng has quickly expanded to a dozen of other provinces or cities including Yunnan, Xinjiang, Inner Mongolia, Gansu, Qinghai, Ningxia, and Shaanxi. The national annual production capacity has increased from the value of 420,000 tons by the end of the 80s to a value of 640,000 tons in mid-1990s. The region with the fastest growing includes Inner Mongolia, Gansu, and Xinjiang region at northwest of China. The production capacity has reached 200,000 tons in Inner Mongolia, which has become the largest production base of sodium sulfide in China. Figure 1 is a picture of yellow flaky sodium sulfide The above information is edited by the lookchem of Dai Xiongfeng.

Industrial sodium sulfide

Industrial sodium sulfide is generally a mixture with different numbers of crystalline water; the molecular formula is Na2S ? nH2O; it exhibits as yellow or reddish-brown massive, flaky and granular and is mainly used in paper, dyes, mineral processing, printing and dyeing industries. GB/T 10500-2000 standard has classified the industrial sodium sulfide products into three categories: Category 1 is ordinary sodium sulfide (commonly known as red base); Class 2 is low-iron sodium sulfide (commonly known as the yellow base); Class 3 is sodium sulfide of high content. Figure 2 the reference quality indicators of industrial sodium sulfide Packing, storage and shipping: sodium sulfide belongs to alkaline corrosive substances, classification: GB 8.2 class, number:82011. It is packed with a tight leakproof iron drums with the net weight per barrel being 25.50 kg or 100 kg. The packaging should contain obvious "drugs" and "corrosive substance" signs. It should be stored in a dry, airy shed asbestos with the container must be intact. It can’t be stored and shipped together with acidic materials and oxidizing agents.

Toxicity

Sodium sulfide is strongly corrosive to the skin. Worker subjecting to contact with a solution of sodium sulfide has their hand skin get ruffling and redness. During the operation, you should note that: upon inadvertently contact with skin, you should rinse with water. After the sodium sulfide droplets or small pieces falling into eyes, immediately wash with water for 15 min and send to hospital for treatment. To protect the skin, it is recommended to wash hands with a weak acetic acid solution and then coated with oily ointment. Pay attention to the protection of eye.

Preparation of polyarylene sulfide

We can take industrial sodium sulfide and poly-halogenated aromatic compounds as raw materials; apply multi-component composite catalyst or additive and carry out segmented poly-condensation at normal pressure in high-boiling polar organic solvent (such as hempa) for generating linear high molecular weight polyarylene sulfide. The reaction conversion rate is high with the product being white granular and with excellent mechanical properties, thermal properties and thermal processing stability. Additionally supplement of a certain amount of cross-linking agent can generate higher molecular weight branched or cross-linked polyarylene sulfide.

Production method

Pulverized coal reduction method: put mirabilite and coal powder in a mixing ratio of 100: (21 to 22.5) (weight ratio) for calcination and reduction at 800~1100 ℃. The resultant after cooling is molten into a liquid. After standing for clarification, the upper portion of the alkaline solution was concentrated to obtain a solid sulfide. The flake (or granules)-like sodium sulfide is made through the transition tank and flaking. The reaction equation is as below: Na2SO4 + 2C → Na2S + 2CO2 Absorption method: use 380~420 g/L sodium hydroxide solution to absorb H2S> 85% containing hydrogen sulfide waste gas; the resulting product was concentrated by evaporation to obtain sodium sulfide products. Its reaction equation is as below: H2S + 2NaOH → Na2S + 2H2O Barium sulfide method: use sodium sulfide and barium sulfide for cross-metathesis reaction to get precipitated barium sulfate. During this process, we can get the byproduct sodium sulfide. The reaction formula is as below: BaS + Na2SO4 → Na2S + BaSO4 ↓ Gas reduction method: in the presence of iron catalyst, put hydrogen (or carbon monoxide, coal gas, methane gas) into boiling furnace for reaction with sodium sulfate, we can obtain high-quality anhydrous granular sodium sulfide (containing Na2S: 95%~97% ). Its reaction equation is: Na2SO4 + 4CO → Na2S + 4CO2 Na2SO4 + 4H2 → Na2S + 4H2O Refined method using the byproduct (4% of sodium sulfide) during the production of precipitated barium sulfate as raw material, pump it into dual-effect evaporator for concentration into 23%; it further enters into the mixing tank for removing iron as well as carbon; pump it into the evaporator (manufactured by pure nickel material) to evaporate the lye into a certain concentration and further send it into the roller squeezing apparatus for flaking and further obtain the finished product after screening and packaging. Pulverized coal reduction method is the traditional production method for making sodium sulfide. During the manufacturing process, improve the equipment and materials and increase the iron removal process so that the products can meet standards.

Toxicity grading

highly toxic

Acute toxicity

oral-rat LD50: 208 mg/kg; Oral-Mouse LD50: 205 mg/kg

Hazardous characteristics of explosive

it is explosive upon heating and collision.

Flammability and hazard characteristics

it release toxic hydrogen sulfide gas upon acids; anhydrous sodium sulfide is flammable; heating can release toxic fumes of sulfur oxides

Storage characteristics

Treasury: ventilation, low-temperature and dry; store it separately from oxidants and acids

Extinguishing agent

water, sand

Preparation

Sodium sulfide is prepared by heating sodium bisulfate with sodium chloride and coal above 950°C. The product mixture is extracted with water and the hydrated sulfide is obtained from the solution by crystallization: NaHSO4 + NaCl + 2C → Na2S + 2CO2↑ + HCl↑Sodium sulfide also is produced from its elements in liquid ammonia: Na + 2S → Na2S.

Air & Water Reactions

Aqueous solutions of sodium sulfide when exposed to air slowly convert to sodium hydroxide and sodium thiosulfate. The crystalline form upon exposure to air forms hydrogen sulfide and sodium carbonate [Merck 11th ed. 1989].

Reactivity Profile

SODIUM SULFIDE is a white to yellow crystalline material, flammable. Can explode on rapid heating or when shocked. Violent reaction with carbon, charcoal, diazonium salts, N,N-dichloromethylamine, strong oxidizers, water. On contact with acids Sodium sulfide liberates highly toxic and flammable hydrogen sulfide gas. When heated to decomposition Sodium sulfide emits toxic fumes of sodium oxide, and oxides of sulfur [Bretherick, 5th ed., 1995, p. 1729].

Hazard

Flammable, dangerous fire and explosion risk. Strong irritant to skin and tissue, liberates toxic hydrogen sulfide on contact with acids.

Health Hazard

Caustic action on skin and eyes. If ingested may liberate hydrogen sulfide in stomach.

Fire Hazard

Special Hazards of Combustion Products: Irritating sulfur dioxide is produced in fire.

Flammability and Explosibility

Nonflammable

Safety Profile

A poison by ingestion and intraperitoneal routes. Flammable when exposed to heat or flame. Unstable and can explode on rapid heating or percussion. Reacts violently with carbon, diazonium salts, n,n-dichloromethylamine, onitroaniline diazonium salt, water. When heated to decomposition it emits toxic fumes of SOx and Na2O. See also SULFIDES

Purification Methods

Some purification of the hydrated salt can be achieved by selecting large crystals and removing the surface layer (contaminated with oxidation products) by washing with distilled water. Other metal ions can be removed from Na2S solutions by passage through a column of Dowex ion-exchange A-1 resin, Na+-form. The hydrated salt can be rendered anhydrous by heating it in a stream of H2 or N2 until water is no longer evolved. (The resulting cake should not be heated to fusion because it is readily oxidised.) Recrystallise it from distilled water [Anderson & Azowlay J Chem Soc, Dalton Trans 469 1986]. Note that sodium sulfide hydrolyses in H2O to form NaHS + H2O, and is therefore alkaline. A 0.1N solution in H2O is 86% hydrolysed at room temperature. Its solubility in H2O is 8% at 0o, 12% at 20o and 30% at 50o. The anhydrous salt is obtained by allowing it to stand in a vacuum over conc H2SO4 or P2O5 at 45o to start with, then at 30-35o when the salt contains 4% of water. The last traces of water are removed by heating to 700o in a glass or porcelain tube in a stream of H2 to give pure H2S. [Fehér in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 358-360 1963.]

InChI:InChI=1/2Na.S/rNa2S/c1-3-2

Upstream product

• 534-18-9 sodium trithiocarbonate 
• 463-58-1 carbon oxide sulfide 
• 1310-73-2 sodium hydroxide 
• 497-19-8 sodium carbonate 
• 7757-82-6 sodium sulfate 
• 17341-25-2 sodium cation 
• 7446-09-5 sulfur dioxide 
• 7440-23-5 sodium 
• 7439-89-6 iron 
• 10025-67-9 disulfur dichloride 
• 7783-06-4 hydrogen sulfide 

Downstream Products

• 7704-34-9 sulfur 
• 14808-79-8 Sulfate 
• 14265-45-3 sulfite^(2-) 
• 14383-50-7 thiosulphate ion 
• 26041-18-9 sulfide ion 
• 651-84-3 4-trifluoromethyl-2,3,5,6-tetrafluorothiophenol 
• 22868-13-9 sodium disulfide 
• 37488-76-9 sodium trisulfide 
• 25326-93-6 monothiomolybdate^(2-) 
• 16608-22-3 dithiomolybdate^(2-) 
• 19452-56-3 trithiomolybdate^(2-) 
• 16330-92-0 tetrathiomolybdate(VI) 
• 858844-31-2 {(cyclo-C₆H₁₁)3}GeSSGe{(cyclo-C₆H₁₁)3} 
• 13634-93-0 4-chloro-2,3,5,6-tetrafluorobenzenethiol 

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Relevant articles and documents

Complex Hydroxides of Chromium: Na9[Cr(OH)6]2(OH)3 ? 6 H2O and Na4[Cr(OH)6]X ? H2O (X = Cl, (S2)1/2) - Synthesis, Crystal Structure, and Thermal Behaviour

Green plate-like crystals of Na9[Cr(OH)6]2(OH)3 · 6H2O (triclinic, P1?, a = 872.9(1) pm, b = 1142.0(1) pm, c = 1166.0(1) pm, α = 74.27(1)°, β = 87.54(1)°, γ = 70.69(1)°) are obtained upon slow cooling of a hot saturated solution of CrIII in cone. NaOH (50 wt%) at room temperature. In the presence of chloride or disulfide the reaction yields green prismatic crystals of Na4[Cr(OH)6]Cl · H2O (monoclinic, C2/c, a = 1138.8(2) pm, b = 1360.4(1) pm, c = 583.20(7) pm, β = 105.9(1)°) or green elongated plates of Na4[Cr(OH)6](S2)1/2 · H2O (monoclinic, P21/c, a = 580.8(1) pm, b = 1366.5(3) pm, c = 1115.0(2) pm, β = 103.71(2)°), respeclively. The latter compounds crystallize in related structures. All compounds can be described as distorted cubic closest packings of the anions and the crystal water molecules with the cations occupying octahedral sites in an ordered way. The thermal decomposition of the compounds was investigated by DSC/TG or DTA/TG and high temperature X-ray powder diffraction measurements. In all cases the final decomposition product is NaCrO2.

Na3+xMxP1?xS4 (M = Ge4+, Ti4+, Sn4+) enables high rate all-solid-state Na-ion batteries Na2+2δFe2?δ(SO4)3|Na3+xMxP1?xS4|Na2Ti3O7

Electrolytes in current Na-ion batteries are mostly based on the same fundamental chemistry as those in Li-ion batteries-a mixture of flammable liquid cyclic and linear organic carbonates leading to the same safety concerns especially during fast charging. All-solid-state Na-ion rechargeable batteries utilizing non-flammable ceramic Na superionic conductor electrolytes are a promising alternative. Among the known sodium conducting electrolytes the cubic Na3PS4 phase has relatively high sodium ion conductivity exceeding 10?4 S cm?1 at room temperature. Here we systematically study the doping of Na3PS4 with Ge4+, Ti4+, Sn4+ and optimise the processing of these phases. A maximum ionic conductivity of 2.5 × 10?4 S cm?1 is achieved for Na3.1Sn0.1P0.9S4. Utilising this fast Na+ ion conductor, a new class of all-solid-state Na2+2δFe2?δ(SO4)3|Na3+xMxP1?xS4 (M = Ge4+, Ti4+, Sn4+) (x = 0, 0.1)|Na2Ti3O7 sodium-ion secondary batteries is demonstrated that is based on earth-abundant safe materials and features high rate capability even at room temperature. All-solid-state Na2+2δFe2?δ(SO4)3|Na3+xMxP1?xS4|Na2Ti3O7 cells with the newly prepared electrolyte exhibited charge-discharge cycles at room temperature between 1.5 V and 4.0 V. At low rates the initial capacity matches the theoretical capacity of ca. 113 mA h g?1. At 2C rate the first discharge capacity at room temperature is still 83 mA h per gram of Na2+2δFe2?δ(SO4)3 and at 80 °C it rises to 109 mA h per gram with 80% capacity retention over 100 cycles.

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Selective and Facile Synthesis of Sodium Sulfide and Sodium Disulfide Polymorphs

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Flux Synthesis of LiAuS and NaAuS: Chicken-Wire-Like Layer Formation by Interweaving of (AuS)nn- Threads. Comparison with α-HgS and AAuS (A = K, Rb)

From the reaction of Au with alkali metal polysulfide liquids, LiAuS and NaAuS were discovered. Orange crystals of LiAuS crystallize in the monoclinic space group C2/c, (no. 15), with a = 8.994(2) ?, b = 8.956(2) ?, c = 7.201(3) ?, β= 128.68(1)°, and Z = 8. Light-yellow planks of NaAuS crystallize in the orthorhombic space group Ccca, (no. 68), with a = 14.658(5) ?, b = 21.043(7) ?, c = 7.118(4) ?, and Z = 32. Both compounds contain infinite one-dimensional (AuS)nn- chains, featuring alternating sulfide anions and linear coordinated Au centers. In LiAuS, the chains are zigzag and fully extended and they pack in two mutually perpendicular sets. In NaAuS, the same chains coil in an unusual fashion so that they become interwoven to form layers reminiscent of chicken-wire . This novel coiling mode allows Au-Au contacts to form, which help to stabilize the structure. The structural relationships between LiAuS, NaAuS, Na7Au5S6, AAuQ (A = K, Rb, Cs; Q = S, Se), and α-HgS are explored.

Kinetics and Mechanism of the Reaction of the Ammoniated Electron with Sodium Thiosulfate in Liquid Ammonia

The reaction of sodium with thiosulfate in liquid ammonia was found to be second order, first order with respect to both the sodium and thiosulfate concentration.The sodium ion concentration was found to have a dominant influence on the net reaction rate, and a mechanism involving ion-paired species is proposed.The stoichiometry and reaction products were also determined.

Synthesis in molten alkali metal polythiophosphate fluxes. The new quaternary bismuth and antimony thiophosphates ABiP2S7 (A = K, Rb), A3M(PS4)2 (A = K, Rb, Cs; M = Sb, Bi), Cs3Bi2(PS4)3, and Na0.16Bi1.28P2S6

The molten alkali metal polychalcogenide flux method was used to prepare the new compounds ABiP2S7 (A = K, Rb), A3M(PS4)2 (A = K, Rb, Cs; M = Sb, Bi), Cs3Bi2 (PS4)3, and Na0.16Bi1.28P2S6. The structural diversity in this family of compounds ranges from the one-dimensional non-centrosymmetric chains of A3M(PS4)2 and the layered compounds, ABiP2S7 and Cs3Bi2 (PS4)2, to the dense three-dimensional framework of Na0.16Bi1.28P2S6. Their synthesis, structural characterization, optical absorption and thermal properties are reported.

Na2EuAs2S5, NaEuAsS4, and Na4Eu(AsS4)2: Controlling the valency of arsenic in polysulfide fluxes

The reactivity of europium with As species in Lewis basic alkali-metal polysulfide fluxes was investigated along with compound formation and the As3+/As5+ interplay vis-a-vis changes in the flux basicity. The compound Na2EuAs2S5 containing trivalent As3+ is stabilized from an arsenic-rich polysulfide flux. It crystallizes in the monoclinic centrosymmetric space group P21/c. Na2EuAs2S5 has [As2S 5]4- units, built of corner sharing AsS3 pyramids, which are coordinated to Eu2+ ions to give a two-dimensional (2D) layered structure. A sodium polysulfide flux with comparatively less arsenic led to the As5+ containing compounds NaEuAsS4 (orthorhombic, Ama2) and Na4Eu(AsS 4)2 (triclinic, P1) depending on Na2S/S ratio. The NaEuAsS4 and Na4Eu(AsS4)2 have a three-dimensional (3D) structure built of [AsS4]3- tetrahedra coordinated to Eu2+ ions. All compounds are semiconductors with optical energy gaps of ～2 eV.

Mixed thio/oxo orthovanadates Na3[VSxO4-x] (x = 2, 3): Synthesis - crystal structures - properties

Mixed sodium thio/oxo orthovanadates(V), dark red Na3[VS 3O] and orange red Na3[VS2O2], were synthesized via reactions in the melt starting from V, Na, Na2S, Na2O and sulfur. The structure of the low temperature phase of Na3[VS3O] (space group Pnma, a = 589.5(3), b = 962.8(5), c = 1186.6(6) pm, Z = 4, R1 = 0.0494) contains anions [VS3O] 3- almost identical to those known from the high temperature form, β-Na3[VS3O] (space group Cmc21, a = 968.4(4), b = 1194.6(4), c = 590.5(2) pm, Z = 4, R1 = 0.0291). The second order phase transition between these two forms at 536°C was studied by temperature dependent powder diffraction and explained on the basis of a comparison of the anion packing in the two related structures. The packing of the dithiodioxovanadate anions in Na3[VS2O2] (space group Pbca, a = 1162.7(2), b = 592.71(12), c = 1766.7(4) pm, Z = 8, R1 = 0.0312) is also closely related. The chemical bonding in the anions [VS 3O]3- and [VS2O2]3- of approximately ideal C3v and C2v symmetry is discussed on the basis of FP-LAPW band structure calculations and force constants obtained from Raman spectroscopy. The decrease of the calculated band gaps with increasing S content x in Na3[VSxO4-x] is in accordance with the optical properties showing a gradually deepening of the crystal and solution colour. Discernible trends in the chemical bonding in this series of mixed thio-oxo anions also include the amount of π bonding of the V-O and V-S bonds and the corresponding variation of force constants and V-O/V-S distances.

An efficient method for synthesizing dimethylsulfonio-34S-propionate hydrochloride from 34S8

Dimethylsulfoniopropionate (DMSP, (2-carboxyethyl)dimethylsulfonium) is a highly abundant compound in marine environments. As a precursor to the climatically active gas, dimethylsulfide (DMS), DMSP connects the marine and terrestrial sulfur cycles. However, the fate of DMSP in microbial biomass is not well understood as only a few studies have performed isotopic labeling experiments. A previously published method synthesized 34S-labeled DMSP from 34S8, but the efficiency was only 26% and required five separate reactions, expensive reagents, and purification of the products of each reaction. In this study, a method of synthesizing 34S-labeled DMSP from 34S8 is described. Improvements include elemental steps, inexpensive reagents, purification of only one intermediate, and less time to complete. The efficiency of this method is 65% and results in pure DMSP with more than 98% isotope enrichment as determined by 1H-nuclear magnetic resonance (NMR) and gas chromatography–mass spectrometry (GC–MS).