NEUTRALIZATION OF SELECT ACIDS & BASES |
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Neutralization of strong acids and bases can reduce the size of your laboratory's aqueous waste stream. Neutralization is the most efficient and least costly way of managing waste acids and bases. After neutralization, waste liquids can be disposed of to the sanitary sewer.
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Solutions That Should Not Be Neutralized
Acids that are very reactive with water should not be neutralized, unless you have expertise in handling them. These include: acid anhydrides and chlorides; chlorosulfonic acid, fuming nitric and sulfuric acids; liquid halides of boron, silicon, tin, titanium and vanadium; and liquid halides and oxyhalides of phosphorus, selenium and sulfur. Due to safety considerations, you should not attempt to neutralize hydrofluoric acid.
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Personal Protection and Equipment
Carry out neutralizations in a well-ventilated fume hood. Use the sash or a safety shield for protection against vigorous reactions. Wear a chemical resistant apron, splash-proof goggles or a full-face shield and nitrile gloves. Long gloves or gauntlets are also recommended. A five gallon polyethylene bucket is recommended for neutralizing 1-10 liters. A large container is needed in acid neutralization for addition of ice and base, and to safely stir the reaction. |
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PROCEDURES
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Neutralization of Strong Bases
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Neutralization of Strong Acids 1. Prepare a 6 N solution of sodium hydroxide (240 g/L) or potassium hydroxide (336 g/L). 2. One liter of 6 N base can neutralize:
3. Dilute the acid to a 5% (by weight) concentration or less (add acid to water, NOT water to acid). Use ice as necessary to cool the solution. Limit the solution to a maximum of 10 liters. Acids may generate heat upon neutralization. 4. Neutralize with 6 N sodium hydroxide or potassium hydroxide, adding it slowly. 5. Monitor pH with pH paper, a pH meter, or a suitable indicator.6. When pH is between 6 and 9, wash solution down the sanitary sewer using 20 parts water. |