Difference between revisions of "Sodium bicarbonate"
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'''Sodium bicarbonate''', '''sodium hydrogen carbonate''', '''bicarbonate of soda''', '''Bicarb''', or '''baking soda''', is a commonly used reagent with the chemical formula NaHCO<sub>3</sub>. Generally appearing as a fine white powder or fine crystals, sodium bicarbonate is an [[amphoteric]] compound, fulfilling roles as both an acid and a base in different chemical reactions, though it is more often thought of as a base. | '''Sodium bicarbonate''', '''sodium hydrogen carbonate''', '''bicarbonate of soda''', '''Bicarb''', or '''baking soda''', is a commonly used reagent with the chemical formula NaHCO<sub>3</sub>. Generally appearing as a fine white powder or fine crystals, sodium bicarbonate is an [[amphoteric]] compound, fulfilling roles as both an acid and a base in different chemical reactions, though it is more often thought of as a base. | ||
Revision as of 19:41, 15 February 2016
Sodium bicarbonate, sodium hydrogen carbonate, bicarbonate of soda, Bicarb, or baking soda, is a commonly used reagent with the chemical formula NaHCO3. Generally appearing as a fine white powder or fine crystals, sodium bicarbonate is an amphoteric compound, fulfilling roles as both an acid and a base in different chemical reactions, though it is more often thought of as a base.
Contents
Properties
Chemical
Sodium bicarbonate will react with acids to release carbon dioxide.
- NaHCO3 + HX → H2O + CO2 + NaX
Sodium bicarbonate reacts with bases such as sodium hydroxide to form carbonates:
- NaHCO3 + NaOH → Na2CO3 + H2O
Sodium bicarbonate slowly decomposes to form sodium carbonate above 50 °C, though the rate of decomposition is much higher at or above 200 °C.
Physical
Sodium bicarbonate forms white crystals and is soluble in water. It has a slightly salty taste, similar to that of sodium carbonate.
Acquisition
Relatively pure sodium bicarbonate can be purchased in supermarkets, cheaply and in large quantities, as baking soda. It is essential to buy unscented baking soda, as scented baking soda may form side products with other reactants or give a nauseating odor in many reactions.
Preparation
Sodium bicarbonate can be prepared by bubbling carbon dioxide in a solution of sodium carbonate.
Uses
Sodium bicarbonate is one of the most versatile and commonly encountered compounds in amateur chemistry. Neutralization of sodium bicarbonate with acids yields a sodium salt and large amounts of carbon dioxide; reaction vessels should have ample headroom to prevent spills. Due to its ease of access and relative cheapness, sodium bicarbonate can be used to neutralize and clean acid spills as well; it is convenient, because the reaction of neutralization in its case is endothermic and results in cooling, unlike with hydroxides, which give very exothermic reactions that may lead to boiling and sprinkling of acids. As many carbonates are not water-soluble, sodium bicarbonate can be used in double replacement reactions to produce the carbonates of many metals.
Sodium bicarbonate, like sodium carbonate, can be used in acid-base titrations.
Handling
Safety
Sodium bicarbonate is non-toxic, but if swallowed it will neutralize the gastric acid and release carbon dioxide, causing burps or if too much is ingested, vomit. It will also increase the sodium level in blood if large quantities are consumed.
Storage
Sodium bicarbonate should be stored in closed bottles away from any acidic vapors.
Disposal
Sodium bicarbonate can be poured down the drain.
