Active Chlorine

Percent active chlorine is a unit of concentration used for hypochlorite-based bleaches. One gram of a 100% active chlorine bleach has the quantitative bleaching capacity as one gram of free chlorine. The term "active chlorine" is used because most commercial bleaches also contain chlorine in the form of chloride ions, which have no bleaching properties.

Liquid bleaches for domestic use fall in 3 categories: for pool-treatment (10% hypochlorite solutions, without surfactants and detergents), for laundry and general purpose cleaning, at 3–5% active chlorine (which are usually recommended to be diluted substantially before use), and in pre-mixed specialty formulations targeted at particular cleaning, bleaching or disinfecting applications. Commercial chlorine bleaches range from under 10% active chlorine to over 40%.

Values can be higher than 100% because hypochlorite ion has a molecular weight of 51.45 g/mol, whereas dichlorine Cl₂ has a molecular weight of 70.90 g/mol. Dichlorine has a reference bleaching potential of 100% for its molecular weight. Hypochlorite (ClO) also has a molecule-to-molecule bleaching potential the same as dichlorine. However, its lower molecular weight leads to a higher potential bleaching power. In the example of lithium hypochlorite, the molecular weight 58.39, so it only takes to equal the bleaching power of of dichlorine. Therefore $70.90 \div 58.39 = 1.214$ or $121.4%$.

Percent active chlorine values have now virtually replaced the older system of chlorometric degrees: 1% active chlorine is equivalent to 3.16 °Cl. Taking the (reasonable) assumption that all active chlorine present in a liquid bleach is in the form of hypochlorite ions, 1% active chlorine is equivalent to 0.141 mol/kg ClO⁻(0.141 mol/L if we assume density=1). For a solid bleach, 100% active chlorine is equivalent to 14.1 mol/kg ClO⁻: lithium hypochlorite has a molar mass of 58.39 g/mol, equivalent to 17.1 mol/kg or 121% active chlorine.

Active chlorine values are usually determined by adding an excess of potassium iodide to a sample of bleach solution and titrating the iodine liberated by displacing it with atomic chlorine with a standard sodium thiosulfate solution and iodine indicator.

Cl2 + 2I- -> I2 + 2 Cl or ClO- + 2I- + 2H+ -> I2 + H2O + Cl-

then

2S2O3^2- + I2 -> S4O6^2- + 2I-

From the above equations it can be seen that 2 moles of thiosulfate is equivalent to of active chlorine.

Again the percentage of available chlorine can be calculated through the concept of normality. The gram equivalent of bleaching powder is equal to the gram equivalent of the standard titrant used.

The amount of available chlorine can then be calculated using the following formula:

$\text \times \frac \times 100 = \text$

References

{{Reflist

*