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In solution, the compound is unstable and easily decomposes, liberating chlorine, which is the active principle of such products. Sodium hypochlorite is still the most important chlorine-based bleach. [10] [11] Its corrosive properties, common availability, and reaction products make it a significant safety risk.
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 ...
Sodium hypochlorite solution, 3–6%, (common household bleach) is typically diluted for safe use when disinfecting surfaces and when used to treat drinking water. [31] [32] A weak solution of 2% household bleach in warm water is typical for sanitizing smooth surfaces before the brewing of beer or wine. [citation needed]
Prepare the Bleach Solution: Mix 1 tablespoon of bleach per 1 gallon of water in a large basin or sink. (Ensure the bleach is unscented and food-safe.) Sanitize the Containers: ...
Step 1: Mix a solution of one-half teaspoon of concentrated chlorine bleach and one quart of warm water in a glass or plastic bowl. Step 2: Add the sponge and be sure it is fully saturated. Step 3 ...
For example, the label of a household bleach product may specify "5% sodium hypochlorite by weight." That would mean that 1 kilogram of the product contains 0.05 × 1000 g = 50 g of NaClO. A typical oxidation reaction is the conversion of iodide I − to elemental iodine I 2. The relevant reactions are NaClO + 2 H + + 2 I − → NaCl + H 2 O ...