Reaction between NaCl and NaHCO3 [closed]








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Does NaHCO3 (aq) react with NaCl(aq)? I don't think they should undergo any reaction but in the online database it is showing that they react to form Na2CO3 and HCl. Is it correct?




Use other online databases, unless you have misinterpreted the database info. Quoting the info would help.


Mixing $\ce{Na2CO3}$ and $\ce{HCl}$ leads to the possibly violent reaction releasing big volume of CO2.


$$\ce{Na2CO3(aq) + HCl(aq) -> H2O(l) + CO2(g) + 2 NaCl(aq)}$$


Be aware that $\ce{NaHCO3(aq)}$ and $\ce{NaCl(aq)}$ mean $\ce{Na+(aq)}$, $\ce{HCO3−(aq)}$ and $\ce{Cl−(aq)}$, all being present side by side in sea water and human blood.


$\ce{HCO3−(aq)}$ does not react with $\ce{Na+(aq)}$ nor $\ce{Cl−(aq)}$, but it does react with water via several acido-basic reactions:


\begin{align}
\ce{HCO3-(aq) + H2O(l) &<=> H2CO3(aq) + OH-(aq)}\\
\ce{HCO3-(aq) &<=> CO3^2-(aq) + H+(aq)}\\
\ce{H+(aq) + OH-(aq) &<=> H2O(l)}
\end{align}


The fact that there are present ions $\ce{Na+(aq)}$, $\ce{CO3^2−(aq)}$, $\ce{H+(aq)}$ and $\ce{Cl−(aq)}$ does not mean there is formed $\ce{Na2CO3}$ and $\ce{HCl}$. Significant presence of $\ce{Na2CO3}$ would mean the solution is strongly alkalic while the same for $\ce{HCl}$ would mean the solution is strongly acidic.


It is neither of that, it is just mildly alkalic because of $\ce{HCO3-(aq)}$. $\ce{CO3^2−(aq)}$ and $\ce{H+(aq)}$ are there just in traces and are independent on $\ce{Na+(aq)}$ and $\ce{Cl−(aq)}$.


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No reaction will occur for those two compounds.


They are both salts that will dissociate in water. The $\ce{HCO\_3^-}$ ion will form a bland ph buffer, but nothing so extreme.


If any molecules of $\ce{HCl}$ will form, they will be instantly dissociated since hydrochloric acid is a strong acid and very soluble in water


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