In my opinion they can't. Because the product of reaction will have $\ce{H2CO3}$, and end up with $\ce{H2O}$ and $\ce{CO2(g)}$. And gas can not be part of a solution.
$$\ce{H2CO3 +2NaHCO3 -> Na2CO3 + 2H2O + 2CO2(g)}$$
$\begingroup$
$\endgroup$
2
-
4$\begingroup$ Well, if you boiled it out and then heated the rest, you would end with Na2CO3(s), H2O(g) and CO2(g). Otherwise, turning drinking water with carbon dioxide/carbonic acid/bicarbonate pH buffer to washing soda solution is not observed. $\endgroup$– PoutnikCommented Jun 20, 2023 at 18:19
-
$\begingroup$ Chem+Math Expression formatting reference: MathJax Basics / Chem+Math expressions/formulas/equations / Upright vs italic / Math SE Mathjax tutorial // MathJax is preferred not to be used in CH SE Q titles. $\endgroup$– PoutnikCommented Jun 20, 2023 at 18:21
Add a comment
|
1 Answer
$\begingroup$
$\endgroup$
There are ongoing four linked equilibrium reactions with their respective equilibrium constants:
$$\ce{CO3^2-(aq) <=>[+H+][-H+]HCO3-(aq)<=>[+H+][-H+]H2CO3(aq)<=>[-H2O][+H2O]CO2(aq)<=>CO2(g)}$$
For drinking water with natural bicarbonate $\mathrm{pH}$ buffer, the concentrations of $\ce{HCO3-(aq)}$ and $\ce{CO2(aq)}$ are comparable, with minor concentration of $\ce{H2CO3(aq)}$. See also carbonic acid on Wikipedia.