Nahco3

Sodium Bicarbonate is buffer commonly used for maintaining the pH of cell culture medium in the presence of 4–10% carbon dioxide. In addition to buffering, sodium bicarbonate provides some nutritional benefit, while rarely displaying any cell toxicity. Formulated as 75 g per liter of water, Gibco™ Sodium Bicarbonate, 7.5% Solution is perfect for supplementing dry powder medium during reconstitution. The final Sodium Bicarbonate concentration used in the medium depends on the media formulation and the carbon dioxide concentration used in the incubator. Product Use For Research Use Only. Not for use in diagnostic procedures. Dual-site cGMP Manufacturing and Quality System Gibco™ Sodium Bicarbonate Solution is manufactured at a cGMP compliant facility, located in Grand Island, New York. The facility is registered with the FDA as a medical device manufacturer and is certified to ISO 13485 standards. For supply chain continuity, we offer an identical Gibco™ Sodium Bicarbonate Solution product made in our Scotland facility (25080-060). This facility is registered with the FDA as a medical device manufacturer and is certified to the ISO 13485 standard.

目录 • 1 化學性质 • 2 制法 • 3 應用 • 4 参见 • 5 參考文獻 • 5.1 引用 • 5.2 来源 • 6 延伸閱讀 • 7 外部連結 化學性质 [ ] 碳酸氢钠是强 127℃以上開始逐漸分解生成 2 NaHCO 3 → Na 2CO 3 + H 2O + CO 2↑ 常利用此特性作為食品制作过程中的膨松剂。 碳酸氢钠可以和酸反应，生成相应的钠盐： NaHCO 3 + 3COOH → 3COONa + H 2O + CO 2↑ NaHCO 3 + HCl → NaCl + H 2O + CO 2↑ 碳酸氢钠溶液可以和镁反应： 4 Mg + 8NaHCO 3 + 4 H 2O → 3MgCO 3·Mg(OH) 2·3H 2O + 4 Na 2CO 3 + 4 H 2↑ + CO 2↑ 制法 [ ] 碳酸氢钠最常见的制备方法是将二氧化碳通入碳酸钠溶液中，结晶得到： Na 2CO 3 + CO 2 + H 2O → 2 NaHCO 3 还有一种方法是，电解饱和食盐水的同时，往其中通入过量二氧化碳 2 NaCl + 2 H 2O + 2 CO 2 - 通电→ 2 NaHCO 3 + Cl 2↑ + H 2↑ 在此反应中，电解生成碳酸氢钠和氯气、氢气。 碳酸氢钠的工业制法为侯氏制碱法： NaCl+NH 3·H 2O+CO 2==NaHCO 3+NH 4Cl 向吸满氨气的饱和食盐水中通二氧化碳，碳酸氢钠溶解度较低，不久后便会沉淀下来 應用 [ ] • 碳酸氫鈉與 • 碳酸氫鈉經常被用作中和劑，例如平衡 • 如在 • 小蘇打可分為藥用、食用、工業用，隨著種類不同在購買地點上也不同。其中，工業用的小蘇打粉的純度較低，雜質較多，相對的食用的小蘇打粉純度較高。 • 小蘇打粉應用於家庭清潔，可以去污、除臭。因油膩、汙漬或難聞氣味，大多屬於酸性物質（H+，如脂肪酸），當弱鹼性的氫氧根OH- 與酸性物質相遇，便會產生中和作用。塗抹髒污靜待數分鐘，之後再輕輕擦拭即可。(不可與醋混和使用) 参见 [ ] • • 參考文獻 [ ] 引用 [ ] 2CO 3 He 2CO 3 3 3 B 3) 2CO 3 4) 2CO 3 4HCO 3 O F Ne 2CO 3 3 2CO 4 3 2(CO 3) 3 Si P S Cl Ar 2CO 3 3 3 3) 2 2(CO 3) 3 Ti V Cr 3 3 3 3 3 2(OH) 2CO 3 3 2(CO 3) 3 Ge As Se Br Kr 2CO 3 3 3 2(CO 3) 3 Zr Nb Mo Tc Ru Rh 3 2CO 3 3 2(CO 3) 3 3 Sb Te I Xe 2CO 3 3 3 镧系 Hf Ta W Re Os Ir Pt Au 2CO 3 3 2CO 3 3 3(OH) 2(CO 3) 2 2O 2CO 3 Po At Rn Fr 3 锕系 Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og ↓ 镧系 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 Pm 2(CO 3) 3 3 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 2(CO 3) 3 锕系 2(CO 3) 3 3) 2 Pa 2CO 3 Np Pu Am Cm Bk Cf Es Fm Md No Lr • （ 英语 ： Internationa...

I had a recent question on a test that asked what the products would be if sodium hydrogen carbonate were dissolved in water. I had a few candidate answers • $\displaystyle\ce$, but that has water on both sides of the equation. Part two of the question asked whether the solution would be acidic, basic, or neutral. What is the proper reaction for this? $\begingroup$ once NaHCO3 is dissolved, the dissolution products are the Na+ ion and the HCO3- ion . According to wikipedia the HCO3- ion reacts with water to produce H2CO3 and a OH- ion, so the solution will be basic. The H2CO3 will decompose into water and carbon dioxide. So I guess that the most likely dissolution reaction will be the 3rd that you proposed $\endgroup$ It's not as intuitive as it seems and your questions are all legitimate questions, but sometimes even good arguments can't be used as evidence in chemistry. $\ce$ will have a higher pH, will become mildly alkaline. First, ionize the salt as you have shown. NaOH is a very strong base so Na+ must be a very weak acid. It is solvated. Being a singly-charged, rather large cation, it stops there. If it were $\ce$, coordinated water would be acidic by charge withdrawal from that brutally small trication. Bicarbonate is the salt of the first ionization of weak carbonic acid. It will then be a modestly weak base by hydrolysis, as you have shown (reversible). Bicarbonate solutions are weakly basic. If you add acid (even weak acetic acid) they fizz. Boiling the solution...

Before taking this medicine Ask a doctor or pharmacist if it is safe for you to take this medicine if you have other medical conditions, especially: • kidney disease; • liver disease; • heart disease; • high blood pressure; or • if you are on a low salt diet. It is not known whether sodium bicarbonate will harm an unborn baby. However, sodium bicarbonate can cause fluid to build up in your body, which may be dangerous during pregnancy. Do not use this medicine without a doctor's advice if you are pregnant. It is not known whether sodium bicarbonate passes into breast milk or if it could harm a nursing baby. Do not use this medicine without a doctor's advice if you are breast-feeding a baby. How should I take sodium bicarbonate? Use exactly as directed on the label, or as prescribed by your doctor. Do not use in larger or smaller amounts or for longer than recommended. Sodium bicarbonate tablets are usually dissolved completely in water before swallowing. Follow al directions on the product label. Call your doctor if your symptoms do not improve, or if they get worse while using sodium bicarbonate. Store at room temperature away from moisture and heat. Sodium bicarbonate side effects Get emergency medical help if you have signs of an allergic reaction: Sodium bicarbonate may cause serious side effects. Stop using sodium bicarbonate and call your doctor at once if you have: • severe stomach • swelling, rapid weight gain; or • shortness of breath (even with mild exertion). Co...

One way to speed up the decomposition of the dry ingredient is by heating it in a warm oven. Baking soda starts to break into washing soda, carbon dioxide, and water at room temperature when mixed with water, which is why you shouldn't store baking soda in an open container or wait too long between mixing a recipe and putting it in the oven. As the temperature increases to the boiling point of water (100 Celcius), the reaction goes to completion, with the decomposition of all the sodium bicarbonate. Helmenstine, Anne Marie, Ph.D. "Equation for the Decomposition of Sodium Bicarbonate (Baking Soda)." ThoughtCo, Aug. 25, 2020, thoughtco.com/decomposition-equation-for-baking-soda-604045. Helmenstine, Anne Marie, Ph.D. (2020, August 25). Equation for the Decomposition of Sodium Bicarbonate (Baking Soda). Retrieved from https://www.thoughtco.com/decomposition-equation-for-baking-soda-604045 Helmenstine, Anne Marie, Ph.D. "Equation for the Decomposition of Sodium Bicarbonate (Baking Soda)." ThoughtCo. https://www.thoughtco.com/decomposition-equation-for-baking-soda-604045 (accessed June 15, 2023).