NaHCO3

炭酸水素ナトリウム sodium bicarbonate

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2015/07/04 04:10:23」(JST)

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炭酸水素ナトリウム
IUPAC名 炭酸水素ナトリウム (Sodium hydrogen carbonate)
別称 重炭酸ナトリウム、重炭酸ソーダ、重曹、ビカ
識別情報
CAS登録番号	144-55-8
PubChem	516892
ChemSpider	8609
UNII	8MDF5V39QO
EINECS	205-633-8
DrugBank	DB01390
KEGG	C12603
MeSH	Sodium+bicarbonate
ChEBI	CHEBI:32139
ChEMBL	CHEMBL1353
RTECS番号	VZ0950000
ATC分類	B05CB04,B05XA02
バイルシュタイン	4153970
SMILES [Na+].OC([O-])=O
InChI InChI=1S/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1  Key: UIIMBOGNXHQVGW-UHFFFAOYSA-M  InChI=1/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1 Key: UIIMBOGNXHQVGW-REWHXWOFAQ
特性
化学式	NaHCO3
精密質量	83.982338573 g mol−1
外観	白色結晶
密度	2.20 g cm−3
融点	50 °C, 323 K, 122 °F (分解)
水への溶解度	103 g/L; 69.3 g/L (0 °C); 236 g/L (100 °C)
log POW	-0.82
酸解離定数 pKa	10.329 6.351 (炭酸)
屈折率 (nD)	1.3344
構造
結晶構造	単斜晶系
薬理学
投与経路	静脈注射, 経口
危険性
MSDS	External MSDS
主な危険性	激しい目のかゆみ
NFPA 704	0 1 0
半数致死量 LD50	4.22 g kg−
関連する物質
その他の陰イオン	炭酸ナトリウム
その他の陽イオン	炭酸水素アンモニウム 炭酸水素カリウム
関連物質	硫酸水素ナトリウム リン酸水素ナトリウム
特記なき場合、データは常温 (25 °C)・常圧 (100 kPa) におけるものである。

炭酸水素ナトリウム（たんさんすいそナトリウム、sodium hydrogen carbonate）、別名重炭酸ナトリウム（じゅうたんさんナトリウム、sodium bicarbonate。重炭酸ソーダ、略して重曹とも）は、ナトリウムの炭酸水素塩である。常温で白色の粉末状である。水溶液のpHはアルカリ性を示すものの、フェノールフタレインを加えても変色しない程度の弱い塩基性である。水には少し溶解し、メタノールにも僅かに溶解するものの、エタノールには不溶。具体的には、水 (0 °C) 100 g につき 6.9 g、水 (20 °C) 100 g につき 9.6 g、メタノール (25 °C) 100 g につき 0.8 g 溶解する。

合成

塩化ナトリウム溶液の電気分解で得られた水酸化ナトリウム溶液に二酸化炭素を反応させて製造する。

NaOH + CO₂ → NaHCO₃

工業的にはソルベー法により多量に製造される。これは炭酸水素ナトリウムの水への溶解度が比較的低いため沈殿することによる複分解反応である。

NaCl+H₂O + NH₃ + CO₂ → NH₄Cl + NaHCO₃↓

また、天然の鉱物を精製しても得られる。日本では旭硝子や東ソーなどが生産している。

反応

ソルベー法の過程で得られた炭酸水素ナトリウムは、焼成することにより炭酸ナトリウムの原料となる。

2NaHCO₃ Na₂CO₃ + CO₂ + H₂O

炭酸水素ナトリウムは両性の化合物で、炭酸の酸解離定数がpK_a1 = 6.3、pK_a2 = 10.3 であるため水溶液は pH = 8.3 程度の弱い塩基性を示す。

HCO₃⁻ + H₂O H₂CO₃ + OH^-, pK_a = 6.3

HCO₃⁻ + H₂O CO₃^2- + H₃O⁺, pK_a = 10.3

酸と反応して炭酸と塩を与え、炭酸は二酸化炭素と水に分解する。

NaHCO₃ + HCl → NaCl + H₂CO₃

H₂CO₃ → H₂O+ CO₂ (気体)

酢酸と反応すると酢酸ナトリウムを与える。

NaHCO₃ + CH₃COOH → CH₃COONa + H₂O + CO₂ (気体)

水酸化ナトリウムと反応して炭酸ナトリウムを与える。

NaHCO₃ + NaOH → Na₂CO₃ + H₂O

熱分解

加熱によって炭酸ナトリウム、二酸化炭素、水の三つの物質に分解する。粉末は270 °C で分解。水溶液は放置しておいても徐々に分解してゆくが65 °C以上で急速に分解する。なお常温・常圧であっても空気中には水分が含まれるため、放置しておくと少しずつ分解していく。

2NaHCO₃ → Na₂CO₃ + H₂O + CO₂

用途

消火剤

粉末化し、流動性付与剤として無水ケイ酸やホワイトカーボンを加え、防湿剤として金属石鹸やシリコーンオイルをコーティングしたものが消火剤として用いられる。消防法施行規則第21条の規定による第一種粉末消火薬剤であり、B火災（油火災）とC火災（電気火災）に適応していることから、BC粉末消火剤とも呼ばれる。

熱分解によって生成されたナトリウムイオンと燃焼反応で生じる遊離基（OH•、H•）が結合することで燃焼の継続を抑制するのが粉末消火薬剤の消火原理である。安価なことから、化学消防車や消防艇の粉末消火装置に用いられる。

2NaHCO₃ → Na₂CO₃ + CO₂ + H₂O

Na₂CO₃ → Na₂O + CO₂

Na₂O + OH• + H• → 2NaOH

また、酸と反応し二酸化炭素を発生するので、泡消火器、酸アルカリ消火器にも用いられる。 鉛蓄電池の電解液（希硫酸）の中和剤としても用いられる。

調理

食品添加物として用いられる。加熱によって分解し二酸化炭素を発生する性質から、ベーキングパウダーなどとして調理に使われる。口中で炭酸ガスを発生させるソーダ飴などには粉末で封入される。ワラビなどの山菜のアク抜き、松の実などの臭み取り、豆を早く煮るため、肉を柔らかくする下ごしらえ、グレープフルーツや夏みかんの強烈な酸味を中和させるために直接かけたり、冷凍エビの食感改善などにも使うことができる。さらには、マクビティに代表されるダイジェスティブビスケット類には、重曹が多く使われている。このように食用ともされることから安全性が高いと見られている。しかし大量に摂取するとアルカローシスなどの問題を引き起こす恐れがあるとされているので、特に幼児が誤食しないように注意する必要はある。合わせて、体重 1 kg 当り約 1.26 g で呼吸器に異常をきたすとのデータもある（ただし、通常の場合これほどの量を摂取することは考え難い）。

pH調整剤

pH調整剤として炭酸水素ナトリウム(重曹)添加の効果が認められている。代謝性アルカローシスは、明らかな血圧降下作用を惹起すると指摘されている。この作用がチアジド系降圧剤の降圧機序の一因子であることが指摘されている。

炭酸水

炭酸水素ナトリウムとクエン酸を混ぜると炭酸ガスが発生し炭酸水となるので飲料としても用いられ、レモンを加えレモンソーダにしたり、砂糖を混ぜサイダーを作るということも可能である。

洗浄・脱臭

研磨効果、鹸化（乳化）効果から、洗剤や洗剤の補助として、ティーカップなどの茶渋落とし、換気扇などの固着した油汚れ・焦げ落としに使用されたりする。重曹は、水質汚染で問題とされるBOD・COD値がなく、環境ホルモンも含まれていないため環境にやさしいとされる。また食品添加物としても使用できるくらい人体に対して安全であることも売りとなっている。 流行の携帯ポットなどは洗いにくい上、洗剤が落ちにくいが、重曹はその点洗い残しがあっても安全である。

洗濯機での使用を禁止しているメーカーもある（重曹が洗濯機内部で詰まり、水漏れや故障の恐れがあるため）。

酸性の臭いに対する脱臭効果があり、肉・魚臭さを消したり、靴箱の脱臭剤などにも使用できる。

最近では練り歯磨きやうがいなどにも使用されることがある。

入浴

天然の温泉に含まれる場合は重曹泉となり、これを模した入浴剤もある。炭酸水素ナトリウムは多くの入浴剤に配合されている。

医薬品

医薬品としては、胃酸過多に対して制酸剤として使われる。ただし胃液には塩酸が含まれているために、炭酸水素ナトリウムは急速に分解し二酸化炭素の気泡が発生する。この気泡が胃を刺激し、さらなる胃液の分泌を促進することが知られている。また点滴剤はアシドーシスの対症療法に用いられる。ただし近位尿細管性アシドーシスに対しては、点滴ではなく経口的に投与し続けることでアシドーシスの補正を行う。なお投与がナトリウムの過剰摂取につながり高ナトリウム血症になることが稀にある。

また、炭酸水素ナトリウムを服用、または、静脈内への水溶液の注射などをすると、尿のpHをアルカリ側に傾けることができる。このため、尿のpHが上がると排泄が速くなるような薬物（例えばフェノバルビタール）を、腎臓から尿中へとより速く排泄させるために炭酸水素ナトリウムを投与する場合がある 。

この他、炭酸水素ナトリウムと無水リン酸二水素ナトリウムを混合した物を、坐剤として直腸内へ挿入することがある。この2つの物質が反応することによって、直腸内で二酸化炭素が発生することを利用して、直腸性便秘（腫瘍などの便の通過障害となる器質的な原因が無く、かつ、大腸の動きが鈍いことも原因ではないタイプの便秘。直腸に便が溜まるタイプの便秘。）の治療に用いられることがある。直腸内で二酸化炭素が発生すると、直腸の粘膜を刺激して、結果として排便を促す効果があるとされている 。 なお、大腸内に二酸化炭素が入り込んでも、いずれ粘膜を通して生体内に吸収されてしまうことが知られている。

臨床応用

• 消化性潰瘍（胃潰瘍、十二指腸潰瘍、吻合部潰瘍）
• 逆流性食道炎（胃食道逆流症）
• ゾリンジャー・エリスン症候群
• 胸焼け（英: heartburn & acid indigestion）

農業・園芸

酸性の土壌の中和に用いれば、アルカリ性の土壌を好む植物の生育がよくなる。農作物や人畜及び水産動植物に害を及ぼす恐れがないことが明らかなものとして、安全性の認められた特定農薬（特定防除資材）の1つであり、有機栽培でもウドンコ病等を防除するために使用される。農薬としてハーモメイトが登録され、一般に販売されている。ただし、炭酸水素ナトリウムは葉を褐変させる薬害が起こりやすいため、より薄い濃度で高い殺菌効果を持つ炭酸水素カリウムの方が多く用いられる。

学習目的の実験

中学理科の「化合物の分解」でよく用いられ、生成する二酸化炭素を石灰水の白濁から、水を塩化コバルト紙の赤変から確認する。この実験を行う際、発生した水が加熱部に流れて試験管が割れるのを防ぐために、加熱する試験管の口を加熱部よりやや下向きにしておく必要がある。また、実験終了の際、加熱をやめる前に加熱している試験管から気体採取用にガラス管をつないであり、その先端が水中にある場合は、ガラス管を水中から出しておく必要がある。これは、加熱をやめ、試験管内部の空気が冷え、気圧が下がった際、ガラス管を通じて水が逆流し、試験管が破損することを防ぐためである。

出典

関連項目

• 炭酸
• 炭酸ナトリウム
• ナトロン
• トロナ
• ベーキングパウダー

外部リンク

• 製品安全デ－タシ－ト（MSDS）重炭酸ナトリウム
• 炭酸水素ナトリウム　理科ねっとわーく（一般公開版） - 科学技術振興機構

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Sodium bicarbonate

Names
IUPAC name Sodium hydrogen carbonate
Other names Baking soda, bicarbonate of soda, nahcolite
Identifiers
CAS Registry Number	144-55-8 Y
ATC code	B05CB04 B05XA02, QG04BQ01
Beilstein Reference	4153970
ChEBI	CHEBI:32139 Y
ChEMBL	ChEMBL1353 Y
ChemSpider	8609 Y
DrugBank	DB01390 Y
EC number	205-633-8
InChI InChI=1S/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1 Y Key: UIIMBOGNXHQVGW-UHFFFAOYSA-M Y InChI=1/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1 Key: UIIMBOGNXHQVGW-REWHXWOFAQ
IUPHAR/BPS	4507
Jmol-3D images	Image
KEGG	C12603 Y
MeSH	Sodium+bicarbonate
PubChem	516892
RTECS number	VZ0950000
SMILES [Na+].OC([O-])=O
UNII	8MDF5V39QO Y
Properties
Chemical formula	NaHCO 3
Molar mass	84.007 g mol−1
Appearance	White crystals
Odor	odorless
Density	2.20 g/cm3
Melting point	50 °C (122 °F; 323 K) (decomposes to sodium carbonate)
Solubility in water	9 g/100 mL 69 g/L (0 °C) 96 g/L (20 °C) 165 g/L (60 °C) 236 g/L (100 °C)
Solubility	0.02 %wt acetone, 2.13 %wt methanol @22 °C. insoluble in ethanol
log P	-0.82
Acidity (pKa)	10.329 6.351 (carbonic acid)
Refractive index (nD)	1.3344
Structure
Crystal structure	monoclinic
Pharmacology
Routes of administration	Intravenous, oral
Thermochemistry
Specific heat capacity (C)	87.61 J/mol K
Std molar entropy (So298)	102 J/mol K
Std enthalpy of formation (ΔfHo298)	-947.7 kJ/mol
Gibbs free energy (ΔfG˚)	-851.9 kJ/mol
Hazards
Main hazards	Causes serious eye irritation
Safety data sheet	External MSDS
NFPA 704	0 0 1
Flash point	incombustible
Lethal dose or concentration (LD, LC):
LD50 (Median dose)	4220 mg/kg ( rat, oral )
Related compounds
Other anions	Sodium carbonate
Other cations	Ammonium bicarbonate Potassium bicarbonate
Related compounds	Sodium bisulfate Sodium hydrogen phosphate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y verify (what is: Y/N?)
Infobox references

Sodium bicarbonate (IUPAC name: sodium hydrogen carbonate) is a chemical compound with the formula NaHCO₃. Sodium bicarbonate is a white solid that is crystalline but often appears as a fine powder. It has a slightly salty, alkaline taste resembling that of washing soda (sodium carbonate). The natural mineral form is nahcolite. It is a component of the mineral natron and is found dissolved in many mineral springs. It is among the food additives encoded by European Union, identified by the initials E 500. Since it has long been known and is widely used, the salt has many related names such as baking soda, bread soda, cooking soda, and bicarbonate of soda. The word saleratus, from Latin sal æratus meaning aerated salt, was widely used in the 19th century for both sodium bicarbonate and potassium bicarbonate. The term is no longer in common usage.

History

The ancient Egyptians used natural deposits of natron, a mixture consisting mostly of sodium carbonate decahydrate, and sodium bicarbonate. The natron was ground up, solvated, and used as paint for hieroglyphics.

In 1791, a French chemist, Nicolas Leblanc, produced sodium carbonate, also known as soda ash. In 1846, two New York bakers, John Dwight and Austin Church, established the first factory to develop baking soda from sodium carbonate and carbon dioxide.

This compound, referred to as saleratus, is mentioned in the novel Captains Courageous by Rudyard Kipling as being used extensively in the 1800s in commercial fishing to prevent freshly-caught fish from spoiling.

Production

Main article: Solvay process

NaHCO₃ is mainly prepared by the Solvay process, which is the reaction of sodium chloride, ammonia, and carbon dioxide in water. Calcium carbonate is used as the source of CO₂ and the resultant calcium oxide is used to recover the ammonia from the ammonium chloride. The product shows a low purity (75%). Pure product is obtained from sodium carbonate, water and carbon dioxide as reported in one of the following reactions. It is produced on the scale of about 100,000 tonnes/year (as of 2001).

NaHCO₃ may be obtained by the reaction of carbon dioxide with an aqueous solution of sodium hydroxide. The initial reaction produces sodium carbonate:

CO₂ + 2 NaOH → Na₂CO₃ + H₂O

Further addition of carbon dioxide produces sodium bicarbonate, which at sufficiently high concentration will precipitate out of solution:

Na₂CO₃ + CO₂ + H₂O → 2 NaHCO₃

Commercial quantities of baking soda are also produced by a similar method: soda ash, mined in the form of the ore trona, is dissolved in water and treated with carbon dioxide. Sodium bicarbonate precipitates as a solid from this method:

Na₂CO₃ + CO₂ + H₂O → 2 NaHCO₃

Mining

Naturally occurring deposits of nahcolite (NaHCO₃) are found in the Eocene-age (55.8–33.9 Mya) Green River Formation, Piceance Basin in Colorado. Nahcolite was deposited as beds during periods of high evaporation in the basin. It is commercially mined using in situ leach techniques involving dissolution of the nahcolite by heated water pumped through the nahcolite beds and reconstituted through a natural cooling crystallisation process.

Chemistry

Sodium bicarbonate is an amphoteric compound. Aqueous solutions are mildly alkaline due to the formation of carbonic acid and hydroxide ion:

HCO−
3 + H₂O → H
2CO
3 + OH⁻

Sodium bicarbonate can be used as a wash to remove any acidic impurities from a "crude" liquid, producing a purer sample. Reaction of sodium bicarbonate and an acid produce a salt and carbonic acid, which readily decomposes to carbon dioxide and water:

NaHCO₃ + HCl → NaCl + H₂CO₃

H₂CO₃ → H₂O + CO₂(g)

Sodium bicarbonate reacts with acetic acid (found in vinegar), producing sodium acetate, water, and carbon dioxide:

NaHCO₃ + CH₃COOH → CH₃COONa + H₂O + CO₂(g)

Sodium bicarbonate reacts with bases such as sodium hydroxide to form carbonates:

NaHCO₃ + NaOH → Na₂CO₃ + H₂O

Sodium bicarbonate reacts with carboxyl groups in proteins to give a brisk effervescence from the formation of CO
2. This reaction is used to test for the presence of carboxylic groups in protein.

Thermal decomposition

Above 50 °C, sodium bicarbonate gradually decomposes into sodium carbonate, water and carbon dioxide. The conversion is fast at 200 °C:

2 NaHCO₃ → Na₂CO₃ + H₂O + CO₂

Most bicarbonates undergo this dehydration reaction. Further heating converts the carbonate into the oxide (at over 850 °C):

Na₂CO₃ → Na₂O + CO₂

These conversions are relevant to the use of NaHCO₃ as a fire-suppression agent ("BC powder") in some dry powder fire extinguishers.

Applications

A list of applications are below.

Pest Control

Used to kill cockroaches. Once consumed, it causes internal organs of cockroaches to burst due to gas collection.

Paint and Corrosion Removal

Sodium bicarbonate is used in a process for removing paint and corrosion called sodablasting; the process is particularly suitable for cleaning aluminium panels which can be distorted by other types of abrasive.

pH Balancer

It can be administered to pools, spas, and garden ponds to raise pH levels.

Mild Disinfectant

It has weak disinfectant properties, and it may be an effective fungicide against some organisms. Because baking soda will absorb musty smells, it has become a reliable method for used-book sellers when making books less malodorous.

Fire extinguisher

Sodium bicarbonate can be used to extinguish small grease or electrical fires by being thrown over the fire, as heating of sodium bicarbonate releases carbon dioxide. However, it should not be applied to fires in deep fryers; the sudden release of gas may cause the grease to splatter. Sodium bicarbonate is used in BC dry chemical fire extinguishers as an alternative to the more corrosive ammonium phosphate in ABC extinguishers. The alkali nature of sodium bicarbonate makes it the only dry chemical agent, besides Purple-K, that was used in large-scale fire suppression systems installed in commercial kitchens. Because it can act as an alkali, the agent has a mild saponification effect on hot grease, which forms a smothering soapy foam.

Cooking

Main article: Leavening agent

Sodium bicarbonate, referred to as "baking soda", is primarily used in cooking (baking), as a leavening agent. It reacts with acidic components in batters, releasing carbon dioxide, which causes expansion of the batter and forms the characteristic texture and grain in pancakes, cakes, quick breads, soda bread, and other baked and fried foods. Acidic compounds that induce this reaction include phosphates, cream of tartar, lemon juice, yogurt, buttermilk, cocoa, vinegar, etc. Natural acids in sourdough can be leavened with the addition of small amounts as well. Sodium bicarbonate can be substituted for baking powder provided sufficient acid reagent is also added to the recipe. Many forms of baking powder contain sodium bicarbonate combined with calcium acid phosphate, sodium aluminium sulphate or cream of tartar.

Sodium bicarbonate was sometimes used in cooking vegetables, to make them softer, although this has gone out of fashion, as most people now prefer firmer vegetables. However, it is still used in Asian and Latin American cuisine to tenderise meats. Baking soda may react with acids in food, including vitamin C (L-ascorbic acid). It is also used in breadings such as for fried foods to enhance crispness.

Heat causes sodium bicarbonate to act as a raising agent by releasing carbon dioxide when used in baking. The carbon dioxide production starts at temperatures above 80 °C. Since the reaction does not occur at room temperature, mixtures (cake batter, etc.) can be allowed to stand without rising until they are heated in the oven.

Neutralisation of acids and bases

Sodium bicarbonate is amphoteric, reacting with acids and bases. It reacts violently with acids, releasing CO2 gas as a reaction product. However, sodium bicarbonate is not recommended for the clean up of acid spills. The heat produced increases the reactivity of the acid, and the large amount of carbon dioxide produced may increase the area of the spill.

A wide variety of applications follows from its neutralisation properties, including reducing the spread of white phosphorus from incendiary bullets inside an afflicted soldier's wounds.

Medical uses

Sodium bicarbonate mixed with water can be used as an antacid to treat acid indigestion and heartburn. It is used as the medicinal ingredient in gripe water for infants.

Intravenous sodium bicarbonate is an aqueous solution that is sometimes used for cases of acidosis, or when there are insufficient sodium or bicarbonate ions in the blood. In cases of respiratory acidosis, the infused bicarbonate ion drives the carbonic acid/bicarbonate buffer of plasma to the left and, thus, raises the pH. It is for this reason that sodium bicarbonate is used in medically supervised cardiopulmonary resuscitation. Infusion of bicarbonate is indicated only when the blood pH is markedly (<7.1–7.0) low.

It is used for treatment of hyperkalemia as it will drive K⁺ back into cells during periods of hypocholermic metabolic alkalosis. Since sodium bicarbonate can cause alkalosis, it is sometimes used to treat aspirin overdoses. Aspirin requires an acidic environment for proper absorption, and the basic environment diminishes aspirin absorption in the case of an overdose. Sodium bicarbonate has also been used in the treatment of tricyclic antidepressant overdose. It can also be applied topically as a paste, with three parts baking soda to one part water, to relieve some kinds of insect bites and stings (as well as accompanying swelling).

Adverse reactions to the administration of sodium bicarbonate can include metabolic alkalosis, edema due to sodium overload, congestive heart failure, hyperosmolar syndrome, hypervolemic hypernatremia, and hypertension due to increased sodium. In patients consuming a high-calcium or dairy-rich diet, calcium supplements, or calcium-containing antacids such as calcium carbonate (e.g., Tums), the use of sodium bicarbonate can cause milk-alkali syndrome, which can result in metastatic calcification, kidney stones, and kidney failure.

Sodium bicarbonate can be used to treat an allergic reaction to plants such as poison -ivy -oak or -sumac to relieve some of the associated itching.

Bicarbonate of soda can also be useful in removing splinters from the skin.

Some alternative practitioners, such as Tullio Simoncini, have promoted baking soda as a cancer cure, which the American Cancer Society has warned against due to both its unproven effectiveness and potential danger in use.

Personal hygiene

Toothpaste containing sodium bicarbonate has in several studies shown to have a better whitening and plaque removal effect than toothpastes without it.

Sodium bicarbonate is also used as an ingredient in some mouthwashes. It has anti-caries and abrasive properties. It works as a mechanical cleanser on the teeth and gums, neutralises the production of acid in the mouth and also acts as an antiseptic to help prevent infections.

Sodium bicarbonate in combination with other ingredients can be used to make a dry or wet deodorant. It may also be used as a shampoo.

Sodium bicarbonate may be used as a buffering agent, combined with table salt, when creating a solution for nasal irrigation.

It is used in eye hygiene to treat blepharitis. This is done by addition of a tablespoon of sodium bicarbonate to cool water that was recently boiled, followed by gentle scrubbing of the eyelash base with a cotton swab dipped in the solution.

In sports

Small amounts of sodium bicarbonate have been shown to be useful as a supplement for athletes in speed-based events, like middle distance running, lasting from about one to seven minutes. However, overdose is a serious risk because sodium bicarbonate is slightly toxic; and gastrointestinal irritation is of particular concern. Additionally, this practice causes a significant increase in dietary sodium.

As a cleaning agent

A paste from baking soda can be very effective when used in cleaning and scrubbing. For cleaning aluminium objects, the use of sodium bicarbonate is discouraged as it attacks the thin unreactive protective oxide layer of this otherwise very reactive metal. A solution in warm water will remove the tarnish from silver when the silver is in contact with a piece of aluminium foil. A paste of sodium bicarbonate and water is useful in removing surface rust as the rust forms a water soluble compound when in a concentrated alkaline solution. Cold water should be used as hot water solutions can corrode steel.

Baking soda is commonly added to washing machines as a replacement for softener and to remove odors from clothes. Sodium bicarbonate is also effective in removing heavy tea and coffee stains from cups when diluted with warm water.

During the Manhattan Project to develop the atomic bomb in the early 1940s, many scientists investigated the toxic properties of uranium. They found that uranium oxides stick very well to cotton cloth, but did not wash out with soap or laundry detergent. The uranium would wash out with a 2% solution of sodium bicarbonate (baking soda). Clothing can become contaminated with depleted uranium (DU) dust, and then normal laundering will not remove it. Those at risk of DU dust exposure should have their clothing washed with baking soda (about 6 ounces (170 g) of baking soda in 2 gallons (7.5 l) of water).

As a biopesticide

Sodium bicarbonate can be an effective way of controlling fungus growth, and in the United States is registered by the Environmental Protection Agency as a biopesticide.

Cattle feed supplements

Sodium bicarbonate is sold as a cattle feed supplement, in particular as a buffering agent for the rumen.

In popular culture

Film

Sodium bicarbonate, as 'bicarbonate of soda', was a frequent source of punch lines for Groucho Marx in Marx brothers movies. In Duck Soup, Marx plays the leader of a nation at war. In one scene, he receives a message from the battlefield that his general is reporting a gas attack, and Groucho tells his aide, "Tell him to take a teaspoonful of bicarbonate of soda and a half a glass of water." In A Night at the Opera, Groucho's character addresses the opening night crowd at an opera by saying of the lead tenor, "Signor Lassparri comes from a very famous family. His mother was a well-known bass singer. His father was the first man to stuff spaghetti with bicarbonate of soda, thus causing and curing indigestion at the same time."

Difference between baking soda and baking powder

Quite simply, baking powder contains baking soda, as well as a powdered acid and cornstarch. In scientific terms, baking soda is a pure substance; baking powder is a mixture.

Baking soda is alkaline, so acid is used in baking powder to avoid a metallic taste when the chemical change during baking creates sodium carbonate. However, to avoid the over-flavouring of acidic taste, non-acid ingredients such as whole milk or Dutch-processed cocoa must be added.

See also

• Carbonic acid
• Irish soda bread
• List of ineffective cancer treatments
• List of minerals
• Nahcolite
• Natron
• Natrona (disambiguation)
• Trona
• Washing soda

Notes

References

Further reading

• Bishop, D; Edge, J; Davis, C; Goodman, C (May 2004). "Induced metabolic alkalosis affects muscle metabolism and repeated-sprint ability". Medicine and science in sports and exercise 36 (5): 807–13. doi:10.1249/01.MSS.0000126392.20025.17. ISSN 0195-9131. PMID 15126714. 
• David R. Lide, ed. (2003). CRC Handbook of Chemistry and Physics (84th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0484-9. 

External links

• International Chemical Safety Card 1044
• Differences between Baking Soda and Baking Powder

UpToDate Contents

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