2014年10月5日 · Acidic water greatly enhances the solubility of calcium carbonate, and it doesn't even need to be highly acidic. Rain or river water that come into contact with the atmosphere absorb the $\ce{CO2}$ as $$\ce{H2O + CO2 <=> H2CO3},$$ which then facilitates calcium carbonate dissolution with $$\ce{CaCO3 + H2CO3 <=> Ca^2+ + 2HCO3-}.$$

2022年9月8日 · Calcium carbonate dissolves by falling apart into ions (calcium cations and carbonate anions): $$\ce{CaCO3(s) <=> Ca^2+(aq) + CO3^2-(aq)}$$ The rate of dissolution does not depend on pH. However, there is a back reaction, which depends on the concentration of the calcium cation and the carbonate anion.

2019年8月2日 · $\begingroup$ "The solubility of CO2 (0.058 g/100mL @ 60 C) would appear to be insufficient to dissolve ~10 g of CaCO3" wrong. One can dissolve way more CO2 in water in presence of CaCO3. Pressure can also be applied and it is good to know at what pressure the solubility is measured. $\endgroup$ –

2024年12月12日 · Your question is complex. the solubility of calcium carbonate in water is about 1mg in 100 ml of [CO2 free] water. the solubility of calcium hydroxide in water is about 185 mg in 100mL of water. A careful preparation of the solid in water followed by centrifugation should give relatively pure CaCO3 and a saturated solution of CaCO3 in a dilute ...

2017年3月14日 · Calcium carbonate will dissolve quickly in a strong acid, like hydrochloric, even if it is dilute and therefore not so dangerous. An organic acid has a problem in that it may have a relatively low pH at first, but after it dissolves a bit of the $\ce{CaCO3}$ , a significant amount of the acid anion is formed in the solution, which stifles the ...

2021年4月4日 · Perhaps the "correct" question to ask is: the equation has 3 degrees of freedom (pH, [carbonate], and [$\ce{CO2}$]). Aquarists add a set amount of carbonate, and measure pH and assume the carbonate doesn't change. This clearly isn't exactly right and that can be seen in the case of pure water exposed to $\ce{CO2}$.

2016年5月27日 · How this influences the solubility depends on the specific system, and is hard to predict. However, there a few salts like cerium sulphate , lithium carbonate sodium carbonate monohydrate, etc. whose solubility decreases with the increase in temperature. How it is so ?

2015年9月5日 · It apparently has a solubility of 16.6 g per 100 mL of water at room temperature. which is about a 1 M solution. Magnesium bicarbonate similarly exists only in aqueous solution, though it is much less soluble at 0.077 g / 100 mL. As solids, these salts probably fall victim to the following equilibrium( $\ce{M}$ is a generic divalent metal:

2016年9月26日 · This will cause a little more calcium carbonate to dissolve than it would in pure water. I'll digress and point out that the solubility product itself really isn't a constant but depends on the ionic strength of the solution. But, off the top of my head, I can't remember if there is a way to calculate [$\ce{Ca^{2+}}$] as a function of [NaCl].

2020年1月11日 · The solubility of $\ce{CaCO3}$ in distilled water is about 15 mg/L, which is about 0.15 mM calcium ion if there is no other source of carbonate. The solubility constant for $\ce{CaF2}$ is about $4\times 10^{-11}$ , which means that we can only have 0.5 mM fluoride ions before precipitation will start.