2016年12月2日 · In application of hydrogen peroxide to soil and groundwater to remediate petroleum contamination, how will the naturally occurring limestone react with the peroxide, thereby reducing the effectiveness of the application. Would calcium peroxide be more suitable.

2015年9月5日 · According to it's Wikipedia page, calcium bicarbonate is not a known solid compound, but it does exist in solution, presumably prepared by dissolving calcium carbonate and bubbling carbon dioxide through the solution until bicarbonate dominates the following pH-dependent disproportionation: $$\ce{2HCO3- <=> H2O + CO2 + CO3^2-}$$

2024年2月23日 · A countertop company (Wilsonart) advises the use of sodium bicarbonate to remove limescale (solid calcium carbonate) from the worktop surface. Acidic solutions are contraindicated because the countertop (which is solid laminate, probably phenolic resin) is sensitive to acid.

2014年10月5日 · As the LE of calcium carbonate is so large, a great amount of free energy would be required to break the strongly attracted ions apart, and this energy has to come from the enthalpy of hydration. In the case of calcium carbonate, the enthalpy of hydration is not large enough to overcome the large lattice energy, hence it exists as a solid.

2016年6月21日 · Hydrogen sulfide react with sodium carbonate to produce sodium bisulfide and sodium bicarbonate. Hydrogen sulfide should be saturated solution. While writing a reaction, you must balance the charges and atoms. In your proposed reaction, where did the carbon go? Indeed, the carbon from sodium carbonate gets converted in the form of sodium ...

2017年4月7日 · $\begingroup$ Phosphoric acid is hydrogen phosphate! If there's a distinction to be made, one can argue that hydrogen phosphate is pure $\ce{H_3PO_4}$, while phosphoric acid is an aqueous solution of hydrogen phosphate (i.e. $\ce{H_3PO_{4\ (aq)}}$). The stoichiometry of the reactions should be the same though. $\endgroup$ –

I could understand the hydrogen ions oxidizing the calcium... Now that would be a very curious reaction. The calcium in calcium carbonate is already in the +2 oxidation state. Calcium has only two valence electrons and further oxidation would require disrupting an intact octet. It would be very unfavorable.

2019年8月2日 · However, the wikipedia page for calcium bicarbonate states that attempts to prepare compounds such as solid calcium bicarbonate by evaporating its solution to dryness invariably yield instead the solid $\ce{CaCO3}$: $\ce{Ca(HCO3)2(aq) → CO2(g) + H2O(l) + …

2015年3月24日 · Nothing is left to balance the carbon in calcium carbonate, so good-bye to that reactant. Nothing is left to balance the calcium in calcium hydroxide, so there can't be that product either. Nothing is left to balance the oxygen in water, so -- no water. And nothing is left to balance the hydrogen in elemental hydrogen gas, so that goes away.

2020年8月14日 · It seems more likely that the precipitate is indeed magnesium carbonate. The water contains 181mg / liter hydrogencarbonate, which is the highest concentration of a molecule in the mains water. The solubility of magensium carbonate is much lower than the solubility of calcium sulfate. (0.14g / liter (MgCO3) vs. 2.1g / liter (CaSO4))