What are the charges of Calcium Carbonate (CaCO3) and Acetic Acid (CH3COOH)?
450621
The compound themselves are neutral but when each compound is dissolve in a solvent (like water), Calcium has a +2 charge, carbonate has a -2 charge, Acetic acid would become acetate (-1 charge) and hydrogen ion (+1 charge).  Hope that helps.
799608
Vinegar is acetic acid,  CH3COOH\n\nCH3COOH + NaHCO3 ---> CH3COONa + H2CO3 (carbonic acid)\n\nThen H2CO3  gives CO2 + H2O  and CO2 will extinguish flame...Many fire extinguishers are made with compressed CO2.
1153335
barium acetate and carbon dioxide and water
290374
Calcium carbonate is a chemical compound, with chemical formula CaCO3.\n\nIt is commonly used as an antacid, and is the active ingredient in agricultural lime. It is a common substance found as rock in all parts of the world and is the main component of seashells and the shell of snails.\nContents\n[hide]\n\n    * 1 Occurrence\n    * 2 Preparation\n    * 3 Chemical properties\n    * 4 Uses\n    * 5 External links\n\n[edit]\n\nOccurrence\n\nCalcium carbonate is found naturally as the following minerals and rocks:\n\n    * Aragonite\n    * Calcite\n    * Chalk\n    * Limestone\n    * Marble\n    * Travertine\n\nEggshells are composed of approximately 95% calcium carbonate.\n\nTo test whether a mineral or rock contains calcium carbonate, strong acids like hydrochloric acid can be dropped with a dropper onto it. If it does contain the chemical, it will fizz and produce carbon dioxide; otherwise, it probably wouldn't react vigorously. For example, all of the rocks/mineral mentioned above will react with acid.\n[edit]\n\nPreparation\n\nThe vast majority of calcium carbonate used in industry is extracted by mining or quarrying. When pure calcium carbonate is required (e.g. for food or pharmaceutical use), it is prepared by passing carbon dioxide into a solution of calcium hydroxide: the calcium carbonate precipitates out, and this grade of product is referred to as precipitated.\n\n    Ca(OH)2 + CO2 → CaCO3 + H2O\n\n[edit]\n\nChemical properties\n\n    See also: Carbonate\n\nCalcium carbonate shares the typical properties of other carbonates. Notably:\n\n   1. it reacts with strong acids, releasing carbon dioxide.\n\n        CaCO3 + 2HCl → CaCl2 + CO2 + H2O\n\n   1. it releases carbon dioxide on heating (to above 825 °C in the case of CaCO3), to form calcium oxide.\n\n        CaCO3 → CaO + CO2\n\nCalcium carbonate will react with water that is saturated with carbon dioxide to form the soluble calcium bicarbonate.\n\n    CaCO3 + CO2 + H2O → Ca(HCO3)2\n\nThis reaction is important in the erosion of carbonate rocks, forming caverns, and leads to hard water in many regions.\n[edit]\n\nUses\n\nThe main use of calcium carbonate is in the construction industry, either as a building material in its own right (e.g. marble) or as an ingredient of cement.\n\nCalcium carbonate is widely used in the pharmaceutical industry, either as an antacid, a calcium supplement (approximately 600 mg of calcium per gram of calcium carbonate), or as a base material for tablets of other pharmaceuticals.\n\nCalcium carbonate is known as whiting in ceramics/glazing applications, where it is used as a common ingredient for many glazes in its white powdered form. When a glaze containing this material is fired in a kiln, the whiting acts as a flux material in the glaze.\n\nIt is commonly called chalk as it has been a major component of blackboard chalk. Chalk may consist of either calcium carbonate or gypsum, hydrated calcium sulfate CaSO4·2H2O.\n\nRecently, calcium carbonate has begun to replace kaolin in the production of glossy paper.\n\nIt is also the substance from which the lens of the mammalian eye is made.\n\nIn 1989, Dr. Simmons introduced CaCO3 into the Whetstone Brook in Massachusetts. His hope was that the calcium carbonate would counter the acid in the stream from acid rain and save the trout that had ceased to spawn. Although his experiment was a success, it did increase the amounts of aluminum ions in the area of the brook that was not treated with the limestone. This shows that CaCO3 can be added to neutralize the affects of acid rain in river ecosystems.\n[edit]\n\nExternal links\n\n    * International Chemical Safety Card 1193\n    * CID 516889 from PubChem
534359
Dilute acetic acid (CH3COOH) is calle as vinegar (I think 30% dilution)\nSince acetic acid is weak acid, its pH will be around 3.5 to 5\n\ndefinately its not 2.4.... \n\nYou can say for vinegar, pH is around 4 to 5
830338
H2CO3 + 2KOH ===> K2CO3 + H2O\n2HNO3 + Ca(OH)2 ===> Ca(NO3)2 + 2H2O
896682
Place a 2 in front of the HCl to balance the equation. Then you can see that for one mole of calcium carbonate, you get 1 mole of carbon dioxide.
88535
Ca(OH)2 \n0.185 g/100cc at 0deg C\n        0.077 g/100cc at 100deg C
812798
3Ca(OH)2+2H3PO4>Ca3(PO4)2+6H2O
551370
Well, the equation is..\nCH3COOH + NaHCO3 ----> CH3COONa (Sodium Acetate) + H2CO3 (Carbonic Acid) \n(or)\nCH3COOH + NaHCO3 ----> CH3COONa (Sodium Acetate) + H2O (Water) + CO2 (Carbon-dioxide)\n\nSo you might have noticed the equation is already balanced. It is a double-displacement reaction. So the sides are already balanced.\nHope this helps.\n\nOne small note...I don't think there is a compound such as NaCO3. The valency of CO3(^-2) ion is 2, so it has to combine with two Sodiums (two positive charges to neutralise its two negative charges) unless the compound one of the above users mentioned is NaCO3-.\n\nrule wid style n luv@vinny
381445
its ca(no3)2, calcium has a charge of positive 2 and nitrate is only negative 1, so you need 2 of them
391116
2Ca(s) + O2(g) -> 2CaO(s)
621890
CaCl2+ 2NaHCO3 + 2H2O------> 2NaCl + 2H2CO3 + Ca(OH)2 \n\n\nyou have to add water molecules on left hand side         \n                                                                                  \nwill this help you?
179442
Depends on what temperature and what other conditions.\n\nDry heating of CaCO3 will result in CaO and CO2 at about 800°C. The CO2 will further go into equilibrium with CO and O2.\n\nAt atmospheric conditions, temperature will influence the solubility of HCO3(1-) in water, and thereby the solution equilibrium.\n\nAt temperatures below freezing, surface ablation by expanding ice crystals can occur.
748691
CH3COOH, remember the CO2 comes from the sodium carbonate so your question is poorly worded.
313942
I forget my organic chem but\n\nammonia, calcium carbonate - a base is used to neutralize an acid - a base donates electrons and an acid collects them (i think, or vs/vs) \n\nboth can be used to separate other chemicals, or remove chemicals from mixtures\n\nAcids are often used as a catalyst to start a reaction like when producing explosives - and can be very dangerous\n\ncommon ex - bleach(acid) mixied with ammonia(base) produce a poisonous gas and heat which can actually cause sever damage to lungs
844699
Egg shells are mostly calcuim carbonate(CaCO3)\n\nso ,the chemical  reaction equation will be :\n\n\n CaCO3(s)+2CH3COOH(aq)-->\nCa(CH3COO)2(aq) +2H2O(l)+CO2(g)