298-14-6 Usage
Chemical Description
Potassium bicarbonate is a white crystalline powder that is used as a fire extinguisher.
Chemical Description
Potassium bicarbonate is a white crystalline powder that is used as a buffering agent.
Uses
Used in Chemical Synthesis:
Potassium bicarbonate is used as a raw material for the production of potassium carbonate, potassium acetate, and potassium arsenite, as well as other compounds.
Used in Medicine:
Potassium bicarbonate is used as a bubbly medication to neutralize stomach acid and boost potassium levels in individuals experiencing severe potassium deficiencies. It has also been employed in studies of renal disorders and the relationship between muscle injury and this process.
Used in Food Industry:
Potassium bicarbonate is used as an acidity regulator and chemical leavening agent in the food industry. It can be added to various types of leavening agents in food products according to production demand.
Used in Pharmaceutical Industry:
Potassium bicarbonate is used in the production of pharmaceuticals, such as antacids and hair/skin products.
Used in Fire Extinguishing:
Potassium bicarbonate serves as an extinguishing agent for oil and chemicals in fire extinguishers.
Used in Agriculture:
Potassium bicarbonate, also known as potassium hydrogen carbonate, is used as a potassium-supplying fertilizer in agriculture. It is a white crystalline solid that decomposes at about 120°C and contains about 28% potassium (K2O).
Used in Research:
Potassium bicarbonate is a widely used reagent in research, employed as a catalyst in synthetic fiber polymerization and olefin dehydrogenation.
Used as a Buffer:
Potassium bicarbonate is used as a buffer in various applications.
Used in Baking Powders and Effervescent Salts:
Potassium bicarbonate is used in baking powders and effervescent salts due to its ability to release carbon dioxide upon heating, providing leavening in baked goods and confectionery products.
Used in Analytical Reagents:
Potassium bicarbonate is commonly used as an analytical reagent in various industries.
Chemical Properties:
Potassium bicarbonate occurs as colorless, transparent crystals or as a white granular or crystalline powder. It is odorless, with a saline or weakly alkaline taste. It is a GRAS (Generally Recognized As Safe) food ingredient, soluble in water but insoluble in alcohol, and stable under normal conditions. Potassium bicarbonate contains no toxic chemicals and is not listed as a carcinogen or potential carcinogen.
Benefits
Sodium bicarbonate and potassium bicarbonate are key components of body tissues that help regulate the body’s acid/base balance. This formula of buffered mineral compounds can assist in reestablishing the acid/base balance when the body’s own bicarbonate reserves are depleted because of metabolic acidosis caused by adverse reactions to food or other environmental exposures.
Potassium is excellent for heart health, If a person does not have enough potassium in the body, a condition known as hypokalemia, negative symptoms can occur. These include fatigue, muscle cramping, constipation, bloating, muscle paralysis and potentially life-threatening heart rhythms, according to the Linus Pauling Institute. Taking potassium bicarbonate can help to reduce these symptoms. Potassium bicarbonate also can lower blood pressure and reduce the risk of developing kidney stones.
Production method
Carbonation way: potassium carbonate can be used as three-grade product as well as alkali as raw materials, including potassium carbonate 40% to 60%, potassium sulfate 10% to 15%, potassium chloride 3.5%. Before feeding, it should be calcined to remove organic matter, taking advantage of the different solubility to remove potassium sulfate and potassium chloride. Addition of lime milk or magnesium carbonate can be used to remove silicon, aluminum, phosphorus and other impurities through pressure filtration. The filtrate, after evaporation, is used for preparation of potassium carbonate solution so that the total alkali concentration is 750~800 g/L (in potassium carbonate) before being sent into the carbonation tower. Carbonization is carried out at a temperature of 50 °C or higher and at a reaction pressure of 0.4 MPa with sending carbon dioxide (concentration of 30% or more). The potassium bicarbonate is continuously precipitated with increasing concentration. After 5~6h carbonation, the mother liquor was separated by crystallization, washed, centrifuged and dried at 80 ℃ to obtain the product of potassium bicarbonate. Its reaction equation is:
K2CO3 + CO2 + H2O → 2KHCO3
Ion exchange method:
The potassium chloride solution is countercurrent passed through the ion exchange column after removing calcium and magnesium, making the (R-Na) be converted into potassium type (RK). Wash with soft water to remove the chloride ions, make the ammonium bicarbonate solution flow downstream through the resin exchange column, obtaining the mixed dilute solution of potassium bicarbonate and ammonium bicarbonate. The dilute solution is mostly decomposed into potassium carbonate after evaporation decomposition. The solution is further sent to the carbonation tower for carbonation of potassium bicarbonate, and then by crystallization, separation, washing and drying to obtain the potassium bicarbonate products. Its
R-Na + KCl → R-K + NaCl
R-K + NH4HCO3 → R-NH4 + KHCO3
2KHCO3 → K2CO3 + CO2 ↑ + H2O
K2CO3 + CO2 + H2O → 2KHCO3
It is obtained through the absorption of carbon dioxide via the 80% ethanol solution of potassium hydroxide or potassium carbonate saturated solution.
K2CO3 + CO2 + H2O → 2KHCO3
Thermal decomposition
The thermal decomposition reactions of potassium bicarbonate dispersed in the KBr pressed disk have been studied by observing the changes in the infrared spectrum of the disk with heating. In the temperature range of 140-220°, the principal reaction in a disk containing up to about 2 mg/g of solute was the decomposition of the cyclic bicarbonate dimer into two monomeric anions with a rate constant of 7.2 x 102 exp[-(14 f 2 kcal)/RT] sec-l. Some carbonate ion was also produced during this reaction, and its yield increased with increasing initial concentration of the solute. At higher reaction temperatures, the formate ion was also produced at a rate second order in the bicarbonate monomer. The rate constant was 7.6 x 10'8 exp [-(49 f 6 kcal)/RT] M-" sec-' for the temperature range 420-500°, and the reaction stoichiometry suggested one formate ion produced from each bicarbonate monomer. The rate of carbonate production in the temperature range 450-550° appeared to be second order in the bicarbonate monomer with an Arrhenius activation energy of about 20 kcal/mol, but quantitative kinetic results could not be obtained for this reaction because of inter-ference by the formate reaction.
References
Thermal Decomposition of Potassium Bicarbonate' by I. C. Hisatsune and T. Ad1
Department of Chemistry, Whitmore Laboratory, The Pennsylvania State Universitg, University Park, Pennsylvania 16802 (Received April 8, 1970)
Toxicity
ADI is not subject to any special provision (FAO/WHO, 2001).
GRAS (FDA, § 184.1613, 2000);
Production Methods
Potassium bicarbonate can be made by passing carbon dioxide into
a concentrated solution of potassium carbonate, or by exposing
moist potassium carbonate to carbon dioxide, preferably under
moderate pressure.
Potassium bicarbonate also occurs naturally in the mineral
calcinite.
Flammability and Explosibility
Nonflammable
Pharmaceutical Applications
Alkali metal carbonates and bicarbonates have wide-ranging pharmaceutical applications. Potassium bicarbonate or citrate is used in over-the-counter drugs as active pharmaceutical ingredients (APIs) against urinary-tract infections (increasing the pH of the urine) in the United Kingdom. Oralbicarbonate solutions such as potassium bicarbonate are typically given orally for chronic acidosis states low pH of the blood plasma. This can be again due to impaired kidney function. The use of potassium bicarbonate for the treatment of acidosis has to be carefully evaluated, as even small changes of the potassium plasma levels can have severe consequences.
Pharmaceutical Applications
As an excipient, potassium bicarbonate is generally used in
formulations as a source of carbon dioxide in effervescent
preparations, at concentrations of 25–50% w/w. It is of particular
use in formulations where sodium bicarbonate is unsuitable, for
example, when the presence of sodium ions in a formulation needs
to be limited or is undesirable. Potassium bicarbonate is often
formulated with citric acid or tartaric acid in effervescent tablets or
granules; on contact with water, carbon dioxide is released through
chemical reaction, and the product disintegrates. On occasion, the
presence of potassium bicarbonate alone may be sufficient in tablet formulations, as reaction with gastric acid can be sufficient to cause
effervescence and product disintegration.
Potassium bicarbonate has also been investigated as a gasforming
agent in alginate raft systems.The effects of potassium
bicarbonate on the stability and dissolution of paracetamol and
ibuprofen have been described.
Potassium bicarbonate is also used in food applications as an
alkali and a leavening agent, and is a component of baking powder.
Therapeutically, potassium bicarbonate is used as an alternative
to sodium bicarbonate in the treatment of certain types of metabolic
acidosis. It is also used as an antacid to neutralize acid secretions in
the gastrointestinal tract and as a potassium supplement.
Safety
Potassium bicarbonate is used in cosmetics, foods, and oral
pharmaceutical formulations, where it is generally regarded as a
relatively nontoxic and nonirritant material when used as an
excipient. However, excessive consumption of potassium bicarbonate
or other potassium salts may produce toxic manifestations of
hyperkalemia.
storage
Potassium bicarbonate should be stored in a well-closed container
in a cool, dry location. Potassium bicarbonate is stable in air at
normal temperatures, but when heated to 100–200°C in the dry
state, or in solution, it is gradually converted to potassium
carbonate.
Purification Methods
It is crystallised from water at 65-70o (1.25mL/g) by filtering and then cooling to 15o (~0.4ml/g). During all operations, CO2 is passed through the stirred mixture. The crystals are sucked dry at the pump, washed with distilled water, dried in air and then over H2SO4 in an atmosphere of CO2. It is much less soluble than the carbonate in H2O (see below).
Incompatibilities
Potassium bicarbonate reacts with acids and acidic salts with the
evolution of carbon dioxide.
Regulatory Status
E501 refers to potassium carbonates). Included in nonparenteral
medicines licensed in the UK and USA (chewable tablets;
effervescent granules; effervescent tablets; lozenges; oral granules;
oral suspensions; powder for oral solutions). Included in the
Canadian List of Acceptable Non-medicinal Ingredients.
Check Digit Verification of cas no
The CAS Registry Mumber 298-14-6 includes 6 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 3 digits, 2,9 and 8 respectively; the second part has 2 digits, 1 and 4 respectively.
Calculate Digit Verification of CAS Registry Number 298-14:
(5*2)+(4*9)+(3*8)+(2*1)+(1*4)=76
76 % 10 = 6
So 298-14-6 is a valid CAS Registry Number.
InChI:InChI=1/CH2O3.K/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1
298-14-6Relevant articles and documents
From K-O2 to K-Air Batteries: Realizing Superoxide Batteries on the Basis of Dry Ambient Air
Chen, Xiaojuan,Qin, Lei,Wu, Yiying,Xiao, Neng,Zhang, Songwei
, p. 10498 - 10501 (2020)
Although using an air cathode is the goal for superoxide-based potassium-oxygen (K-O2) batteries, prior studies were limited to pure oxygen. Now, the first K-air (dry) battery based on reversible superoxide electrochemistry is presented. Spectroscopic and gas chromatography analyses are applied to evaluate the reactivity of KO2 in ambient air. Although KO2 reacts with water vapor and CO2 to form KHCO3, it is highly stable in dry air. With this knowledge, rechargeable K-air (dry) batteries were successfully demonstrated by employing dry air cathode. The reduced partial pressure of oxygen plays a critical role in boosting battery lifespan. With a more stable environment for the K anode, a K-air (dry) battery delivers over 100 cycles (>500 h) with low round-trip overpotentials and high coulombic efficiencies as opposed to traditional K-O2 battery that fails early. This work sheds light on the benefits and restrictions of employing the air cathode in superoxide-based batteries.
Absorption of carbon dioxide into potassium hydroxide: Preliminary study for its application into liquid scintillation counting procedure
Firman, Nur Faiizah Aqiilah,Noor, Alfian,Zakir, Muhammad,Maming,Fathurrahman, Achmad Fuad
, p. 4907 - 4912 (2021/08/31)
This preliminary study presents a theoretical and experimental investigation on the absorption of CO2 into KOH solution. The study provides variation of KOH concentrations at 1, 2, 3, 4, and 5 N. The value of pH was observed for each increment of sample volume. The absorbed CO2 was measured by applying titration. The amounts of CO2 resulted from every provided KOH concentration were respectively 0.0075, 0.0075, 0.0232, 0.0305, and 0.0395 mol. The results reveal an increase in absorbed CO2 with each increment of KOH concentration. The absorption efficiency values of each KOH concentration were 0.3750, 0.4000, 0.3861, 0.3813, and 0.3950 mol total CO2/mol KOH, respectively. The difference values of experimental and theoretical absorbed CO2 may be caused by the formation of other compounds.
The Alkali Metal Salts of Methyl Xanthic Acid
Liebing, Phil,Schmeide, Marten,Kühling, Marcel,Witzorke, Juliane
, p. 2428 - 2434 (2020/06/17)
Methyl xanthates of the type M(SSC-OMe) (M = Li–Cs) are readily formed when carbon disulfide is reacted with the corresponding alkali metal hydroxides in methanol exposed to air, or with the alkali metal methoxides in dry methanol or THF under exclusion of air. The reactions are easily monitored by 13C NMR spectroscopy. The Na, K, Rb, and Cs salt could be isolated in high yields, while the Li salt decomposed upon attempted isolation. All compounds are readily complexed by crown ethers and form isolable 1:1 adducts, including the elusive Li salt. All products were studied by NMR (1H, 13C, and alkali metal nuclei) and IR spectroscopy, and most of them where structurally characterized by single-crystal X-ray diffraction. Li(SSC-OMe)(12c4) (12c4 = [12]crown-4) and Cs(SSC-OMe)(18c6) (18c6 = [18]crown-6) represent the first structurally characterized lithium and caesium xanthate complexes, respectively.
Structural Sensitivities in Bimetallic Catalysts for Electrochemical CO2 Reduction Revealed by Ag-Cu Nanodimers
Huang, Jianfeng,Mensi, Mounir,Oveisi, Emad,Mantella, Valeria,Buonsanti, Raffaella
, p. 2490 - 2499 (2019/03/04)
Understanding the structural and compositional sensitivities of the electrochemical CO2 reduction reaction (CO2RR) is fundamentally important for developing highly efficient and selective electrocatalysts. Here, we use Ag/Cu nanocrystals to uncover the key role played by the Ag/Cu interface in promoting CO2RR. Nanodimers including the two constituent metals as segregated domains sharing a tunable interface are obtained by developing a seeded growth synthesis, wherein preformed Ag nanoparticles are used as nucleation seeds for the Cu domain. We find that the type of metal precursor and the strength of the reducing agent play a key role in achieving the desired chemical and structural control. We show that tandem catalysis and electronic effects, both enabled by the addition of Ag to Cu in the form of segregated nanodomain within the same catalyst, synergistically account for an enhancement in the Faradaic efficiency for C2H4 by 3.4-fold and in the partial current density for CO2 reduction by 2-fold compared with the pure Cu counterpart. The insights gained from this work may be beneficial for designing efficient multicomponent catalysts for electrochemical CO2 reduction.
A Carbon-Neutral CO2 Capture, Conversion, and Utilization Cycle with Low-Temperature Regeneration of Sodium Hydroxide
Kar, Sayan,Goeppert, Alain,Galvan, Vicente,Chowdhury, Ryan,Olah, Justin,Prakash, G. K. Surya
supporting information, p. 16873 - 16876 (2018/11/06)
A highly efficient recyclable system for capture and subsequent conversion of CO2 to formate salts is reported that utilizes aqueous inorganic hydroxide solutions for CO2 capture along with homogeneous pincer catalysts for hydrogenation. The produced aqueous solutions of formate salts are directly utilized, without any purification, in a direct formate fuel cell to produce electricity and regenerate the hydroxide base, achieving an overall carbon-neutral cycle. The catalysts and organic solvent are recycled by employing a biphasic solvent system (2-MTHF/H2O) with no significant decrease in turnover frequency (TOF) over five cycles. Among different hydroxides, NaOH and KOH performed best in tandem CO2 capture and conversion due to their rapid rate of capture, high formate conversion yield, and high catalytic TOF to their corresponding formate salts. Among various catalysts, Ru- and Fe-based PNP complexes were the most active for hydrogenation. The extremely low vapor pressure, nontoxic nature, easy regenerability, and high reactivity of NaOH/KOH toward CO2 make them ideal for scrubbing CO2 even from low-concentration sources - such as ambient air - and converting it to value-added products.
Carbon dioxide as a pH-switch anti-solvent for biomass fractionation and pre-treatment with aqueous hydroxide solutions
To, Trang Quynh,Kenny, Ceire,Cheong, Soshan,Aldous, Leigh
supporting information, p. 2129 - 2134 (2017/07/18)
Rice husks (or rice hulls) pre-treated with aqueous potassium hydroxide solutions showed excellent glucose yields during enzymatic saccharification. CO2 addition to the hydroxide solutions precipitated the dissolved rice husk silica as a nanoporous powder, while Ca(OH)2 addition regenerated the hydroxide solution and precipitated the dissolved lignin. Fractionation of the biomass was thus achieved using CO2 addition as a reversible pH-switch, and the hydroxide could be repeatedly recycled while maintaining biomass pre-treatment and fractionation efficacy.
Process for the preparation of dimethyl ether
-
Page/Page column 3-5, (2009/04/23)
Process for the preparation of dimethyl ether product by catalytic conversion of synthesis gas to dimethyl ether comprising contacting a stream of synthesis gas comprising carbon dioxide with one or more catalysts active in the formation of methanol and the dehydration of methanol to dimethyl ether to form a product mixture comprising the components dimethyl ether, methanol, carbon dioxide and unconverted synthesis gas, washing the product mixture comprising carbon dioxide and unconverted synthesis gas in a scrubbing zone with a liquid solvent being rich in potassium carbonate or amine and thereby selectively absorbing carbon dioxide in the liquid solvent, subjecting the thus treated product mixture to a distillation step to separate methanol and water from dimethyl ether and unconverted synthesis gas stream with a reduced content of carbon dioxide and separating the unconverted synthesis gas from the dimethyl ether product.
PROCESS FOR THE PREPARATION OF DIMETHYL ETHER
-
Page/Page column 2, (2009/04/24)
Process for the preparation of dimethyl ether product by catalytic conversion of synthesis gas to dimethyl ether comprising contacting a stream of synthesis gas comprising carbon dioxide with one or more catalysts active in the formation of methanol and the dehydration of methanol to dimethyl ether to form a product mixture comprising the components dimethyl ether, methanol, carbon dioxide and unconverted synthesis gas, washing the product mixture comprising carbon dioxide and unconverted synthesis gas in a scrubbing zone with a liquid solvent being rich in potassium carbonate or amine and thereby selectively absorbing carbon dioxide in the liquid solvent, subjecting the thus treated product mixture to a distillation step to separate methanol and water from dimethyl ether and unconverted synthesis gas stream with a reduced content of carbon dioxide and separating the unconverted synthesis gas from the dimethyl ether product.
Process for the production of alkylene glycols using homogeneous catalysts
-
Page 11; 12, (2008/06/13)
A process for the manufacture of alkylene glycol by the hydration of alkylene oxide using a soluble catalyst that permits the separation of the reaction product into an alkylene glycol product stream and a recycle stream without the significant precipitation of the soluble catalyst from the recycle stream.
Condensed N-aclyindoles as antitumor agents
-
, (2008/06/13)
The invention provides compounds of general formula (I), wherein: X is halogen or OSO2R, where R represents H or is unsubstituted or hydroxy-or amino-substituted lower alkyl; Y is a nitro or amine group or a substituted derivative thereof; W is selected from the structures of formulae (Ia, Ib or Ic), where E is -N= or -CH=, G is O, S, or NH, and Q is either up to three of R, OR, NRR, NO2, CONHR, NHCOR or NHCONHR, or is an additional group of formulae (Ia, Ib or Ic) and HET represents a 5- or 6-membered carbocycle or heterocycle; and A and B collectively represent a fused benzene or 2-CO2R pyrrole ring. In one embodiment, the group Y is an amine derivative substituted by a group which is a substrate for a nitroreductase or carboxypeptidase enzyme such that one of said enzymes is able to bring about removal of that group.
