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The overall chemical reaction is: CO 2 + Ca(OH) 2 → CaCO 3 + H 2 O + heat (in the presence of water) Each mole of CO 2 (44 g) reacts with one mole of calcium hydroxide (74 g) and produces one mole of water (18 g). The reaction can be considered as a strong-base-catalysed, water-facilitated reaction. [5]
Its solubility product K sp of 5.02 × 10 −6 at 25 °C, [1] its dissociation in water is large enough that its solutions are basic according to the following dissolution reaction: Ca(OH) 2 → Ca 2+ + 2 OH −. The solubility is affected by the common-ion effect. Its solubility drastically decreases upon addition of hydroxide or calcium sources.
Ba(OH) 2 + 2 H + → Ba 2+ + 2 H 2 O. The same equation relating the concentrations of acid and base applies. The concept of neutralization is not limited to reactions in solution. For example, the reaction of limestone with acid such as sulfuric acid is also a neutralization reaction. [Ca,Mg]CO 3 (s) + H 2 SO 4 (aq) → (Ca 2+, Mg 2+)(aq) + SO ...
Ca 0 Calcium: Gas Ca 178.2 Calcium(II) ion Gas Ca 2+ 1925.90 Calcium(II) ion Aqueous Ca 2+ −542.7 Calcium carbide: Solid CaC 2: −59.8 Calcium carbonate Solid CaCO 3: −1206.9 Calcium chloride: Solid CaCl 2: −795.8 Calcium chloride: Aqueous CaCl 2: −877.3 Calcium phosphate: Solid Ca 3 (PO 4) 2: −4132 Calcium fluoride: Solid CaF 2: − ...
Cobalt(II) hydroxide precipitates as a solid when an alkali metal hydroxide is added to an aqueous solution of Co 2+ salt. [4] For example, Co 2+ + 2 NaOH → Co(OH) 2 + 2 Na + The compound can be prepared by reacting cobalt(II) nitrate in water with a solution of triethylamine N(C 2 H 5) 3 as both the base and a complexing agent. [3]
In chemistry, an acid–base reaction is a chemical reaction that occurs between an acid and a base.It can be used to determine pH via titration.Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory.
2 F + Fluoronium ion HF Hydrogen fluoride: HCl Hydrochloric acid: Cl − Chloride ion H 2 SO 4 Sulfuric acid: HSO − 4 Hydrogen sulfate ion (bisulfate ion) HNO 3 Nitric acid: NO − 3 Nitrate ion H 3 O + Hydronium ion H 2 O Water: HSO − 4 Hydrogen sulfate ion SO 2− 4 Sulfate ion H 3 PO 4 Phosphoric acid: H 2 PO − 4 Dihydrogen phosphate ...
The alkali–carbonate reaction is also catalyzed by the soluble NaOH produced by the reaction of Na 2 CO 3 with Ca(OH) 2 (portlandite) present in the hardened cement paste (HCP), therefore perpetuating the reaction indefinitely as observed by Fournier and Bérubé (2000) and Bérubé et al. (2005). [4] [5]