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Oct 5, 2014 · For an ionic substance to dissolve in water, there are two competing factors that determine the enthalpy of solution $\Delta{H}_\mathrm{sol}$ which is the enthalpy (energy) change when a solute is dissolved in a solvent:

Sep 8, 2022 · It is my understanding that calcium carbonate dissolves faster in lower pH environments. I am interested to know how higher PH levels affect the rate of dissolution.

Mar 14, 2017 · $\ce{CaCO3}$ is sedimenting when mixed with water, and therefore is not easy to remove with hot water. . Nevertheless several methods exist that actually dissolve it that are better

Apr 2, 2018 · I am trying to solve an exercise, where a block of 605.5g calcium carbonate should be completely dissolved in 30% hydrochloric acid (w/w) and the concentration of the acid should be 3% in the end. ...

Thermal decomposition of calcium carbonate. In general, we heat $\ce{CaCO3}$ to temperature of approximately 825°C it decomposes into calcium oxide and liberates carbon dioxide gas:* $$\ce{CaCO3} \

Jul 18, 2016 · depends on your equipment. You can estimate the amount of $\ce{NaHCO3}$ by taking a known amount of sample, heating it to $\sim\pu{300 °C}$, cooling it to room temperature and measuring the weight again.

Feb 14, 2014 · $\begingroup$ 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.

Jul 17, 2021 · When $\ce{Ca(OH)2}$ is applied on a wall for whitewashing it reacts with atmospheric $\ce{CO2}$ to give $\ce{CaCO3}$ (and a shiny appearence), but we also learned that, when we pass $\ce{CO2}$ from aqueous solution, $\ce{CaCO3}$ will change into sodium hydrogen carbonate ($\ce{CaHCO3}$) that is soluble in water, so we know $\ce{CaCO3}$ was ...

Oct 22, 2022 · The reaction you write, in aqueous solution, would happen with the ions produced by dissociation of the salts, not with the parent compounds, and would involve not one but two acid-base reactions (with carbonate ion, and then bicarbonate) and finally decomposition of carbonic acid to $\ce{CO2}$.