Introduction
Chlorine is a powerful oxidising agent. It normally occurs as a gas but can be liquefied under pressure at ambient temperatures.
As a dry gas it does not tend to be aggressive towards stainless steels, but as either a damp gas or dissolved in water it can be a corrosion hazard.
Chlorine readily forms chlorides when in contact with gases such as methane, hydrogen sulphide and ammonia. Hydrochloric acid (HCl) can also be formed by these reactions.
Chlorine dissolves readily in water forming hydrochloric and hypochlorous (HOCl) acids, which is very corrosive mixture.
Chlorine can also assist in the oxidation of dissolved gasses, such as sulphur dioxide (SO2), forming sulphuric and hydrochloric acid in water.
It is these oxidising properties that make chlorine an aggressive component in waters.
Corrosion resistance of stainless steels
Chlorine in contact with water and as a dissolved gas, sometimes found in water treatment applications, is potentially aggressive to stainless steels.
Localised crevice & pitting corrosion attack is a hazard in water and stress corrosion cracking (SCC) can be an additional hazard in damp chlorine gas, if the temperature is high enough.
Condensates formed over chlorinated water in storage tanks have been known to result in staining or pitting to stainless steels. Improvements to ventilation in such situations should help reduce the risk of attack.
Chlorine as a sterlizing or sanitising agent
When using chlorine as a sterilizer or sanitiser in contact with 316 type stainless steel items, a maximum of 15-20 ppm (mg/lt) 'free' chlorine is suggested, for maximum times of 24 hours, followed by a thorough chlorine free water flush.
As with any additions, thorough dilution around the injection point is important to avoid localised 'over-concentration' problems.
Residual chlorine levels in waters of 2ppm maximum for 304 and 5ppm for 316 types should not normally be considered a crevice corrosion hazard.
Chlorine dioxide as a sanitiser in contact with stainless steels.
Chlorine dioxide (ClO2), occurs naturally as a gas, but is normally dissolved in water, as the gas is highly explosive.
Although a powerful oxidiser, unlike chlorine it does not breakdown to release chlorides. The chlorine and oxygen work together tending to form chlorites in the oxidation process. Although the chlorite can break down to form chlorides, it is a weaker oxidising agent than the chlorine dioxide and so can be expected to be less of a hazard to stainless steels when used as a water sanitiser.
Source data can be found at Outokumpu Corrosion Handbook - chlorine and chlorine dioxide.
Source: http://www.bssa.org.uk/
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