Registration Dossier

Environmental fate & pathways

Endpoint summary

Administrative data

Description of key information

Additional information

Stability

 

Phototransformation in air

 

If released to air, a vapor pressure of 1.26E-009 mm Hg at 25 deg C (1.26E-009 mm Hg is equivalent to 1.68E-007 Pa ) indicates Sodium isobutyl xanthate will exist solely as a vapor in the atmosphere. Vapor-phase Sodium isobutyl xanthate will be degraded in the atmosphere by reaction with photochemically-produced hydroxyl radicals; the half-life for this reaction in air is estimated to be 0.667 days, calculated from its rate constant of 16.0392 E-12 cm3/molecule-sec at 25 deg.

Xanthates do not contain chromophores that absorb at wavelengths >290 nm and therefore Sodium isobutyl xanthate is not expected to be susceptible to direct photolysis by sunlight.

Using the AOPWIN QSAR model, the photochemical degradation rate of Sodium isobutyl xanthate in the atmosphere is 16.0392 E-12 cm3/molecule-sec, with a resultant predicted half live of 8.002 Hrs (0.667 Days (12-hr day; 1.5E6 OH/cm3)

OVERALL OH Rate Constant = 16.0392 E-12 cm3/molecule-sec

HALF-LIFE = 0.667 Days (12-hr day; 1.5E6 OH/cm3)

HALF-LIFE = 8.002 Hrs

Phototransformation in water

It is not applicable for a compound wich dissociates.

When water is added to Sodium isobutyl xanthate it reacts with water to form the others substances: alcohol, sodium carbonate, trithiocarbonate and carbon disulphide because of its high water solubility.

Phototransformation in soil

If released to soil,Sodium isobutyl xanthate is expected to have very high mobility based upon an estimated Koc of 11.7.

Volatilization from moist soil surfaces is not expected to be an important fate testing for Phototransformation in soils does not need to be performed.

 

Hydrolysis

 

Hydrolysis will be a significant factor in determining the environmental fate of Sodium isobutyl xanthate. In neutral or mildly alkaline solutions, Sodium isobutyl xanthate decomposes to the alcohol, carbon disulphide, sodium carbonate and sodium trithiocarbonate, the two salts arising from neutralisation of carbondisulphide with the sodium hydroxide liberated. In more strongly alkaline media, hydrogen sulphide is liberated. However, strongly alkaline conditions are unlikely to be encountered under the conditions of use in the mining industry. The half-life at pH 7 at 25°C is reportedly about 260 hours, increasing to over 500 hours in the pH range 8 to 11.

Sodium isobutyl xanthate is hydrolytically unstable when exposed to acidic conditions, reverting rapidly to isobutyl, carbon disulphide and caustic soda, and therefore will not persist in the acidic environment of tailings dams. If discharged to waterways, the chemical would be likely to persist for at least some days, hydrolysing only slowly in this more neutral environment. However, it is not expected to bioaccumulate in view of its ionic character.

 

Further hydrolysis of sodium trithiocarbonate to sodium carbonate and hydrogen sulphide and carbon disulphide to carbon dioxide and hydrogen sulphide may occur. The reaction is catalysed by the alcohol formed from the xanthic acid and is self accelerating.

 

On this basis hydrolysis proceed with the others active substances:sodium trithiocarbonate,carbon disulphide,hydrogen sulphide.

 

Xanthates decompose in aqueous solution by dissociation, oxidation and hydrolysis. Hydrolytic decomposition is the main reaction in alkaline solutions while the other two reactions occur in acidic solutions.

 

Aqueous solution

There are three decomposition pathways of xanthates in aqueous solution:

A. Xanthates dissociate forming alkali metal cations and xanthate anions. Thesolution undergoes further hydrolysis to xanthic acid which decomposes intocarbon disulphide and alcohol.

ROCS2Na + H2O→ ROCS2H + NaOH

 

ROCS2H →CS2+ ROH

 

B. Xanthate is oxidised to dixanthogen. The extent of this reaction is very smalland dependent on the pH. Equilibrium is reached after about 5–10% of thexanthate is oxidised, and the reaction increases with a fall in the pH.

 

2ROCS2+ H2O + _O2→ (ROCS2)2+ 2OH

 

C. In neutral and alkaline media, xanthates decompose by hydrolytic decomposition.

6ROCS2+ 3H2O →6ROH + CO32 –+ 3CS2+ 2CS32 –

Further hydrolysis of sodium trithiocarbonate to sodium carbonate andhydrogen sulphide and carbon disulphide to carbon dioxide and hydrogensulphide may occur. The reaction is catalysed by the alcohol formed from thexanthic acid and is self accelerating.

 

Reaction C is the main reaction in alkaline solution while A and B occur in acidic solutions. During use in mining processes, reaction C is the principal decompositionpathway and carbon disulphide the principal decomposition product.

Part of thecarbon disulphide formed may decompose further to carbonate and thiocarbonatesalts, some of it may evaporate and some may build up in the xanthate solution.Once the solubility of carbon disulphide is exceeded it forms a separate layer belowthe sodium isobutyl xanthate solution.

Reactions A and B are minor and require acidic conditions. Reaction C proceeds in neutral or alkaline pH and is self-accelerating, as it is catalysed by the alcohol formed as a product. Its rate increases with concentration of the reagents and with temperature, from 1.1%/day at 20 °C to 4.6%/day at 40 °C for a 10% solution at pH=10. A decrease in pH from 10 to 6.5 increases the decomposition rate from 1.1%/day to 16%/day. Decomposition is also accelerated by the presence of metals, such as copper, iron, lead or zinc, which act as a catalyst