# how to separate a mixture of sodium chloride and sodium hydroxide

I recently did an double displacement reaction in that I have formed a solution of water with sodium hydroxide and sodium chloride are dissolved in it. now I want to separate both of them

• Full separation would be very difficult. So does partial separation $\ce{NaOH}$ from of $\ce{NaCl}$. Partial separation $\ce{NaCl}$ from of $\ce{NaOH}$ is duable, as @Hans says. Oct 22 '20 at 7:44
• Is there some reason you need to recover the NaOH? I would consider neutralizing with HCl to get a solution that is just NaCl and then distill off the water. Nov 28 '20 at 12:55

One solution would be to reduce the amount of solvent (under vacuum for instance), then filter out the precipitated NaCl at high temperature (at higher temperatures NaOH has as much as >10x the water solubility of NaCl).

The common ion effect will play in your favour, as the high water solubility of NaOH at higher temperatures will help you reach NaOH concentrations that strongly disfavours NaCl solubility.

The way to go may be to first reduce the solvent mass under vacuum at acceptably safe temperatures, and once the desired mass is reached redissolving most of the precipitated NaOH by pushing the temperature up before filtration to a level at which most NaOH has redissolved.

Use appropriate protection equipment and contact material to handle very hot NaOH.

• Sorry but concentrated NaOH solutions cannot be filtrated. . Nov 23 '20 at 22:19
• @Maurice: You bring up the point that concentrated NaOH solutions are not as easy to filter as any solution, which is a good remark. Two points on that (1) As for the case here we don't know the proportion of hydroxide vs chloride, so there's no indication how basic the solution would be once concentrated. (2) There are ways even for pure NaOH solutions: a) Cotton + Funnel works well, b) Crystalizing slowly and settling works also, and c) Even in the most extreme cases PTFE membranes with a water miscible solvent (to address the materials hydrophobicity), is another possible solution.
– Hans
Nov 25 '20 at 17:07
• I'm writing this only to balance a remark that fully has its place on the topic.
– Hans
Nov 25 '20 at 17:08

Hans' idea (evaporation + filtration) is not easy to carry out in practice. Concentrated $$\ce{NaOH}$$ solutions are extremely viscous, and if they are mixed with $$\ce{NaC}$$l crystals, they cannot be filtered easily. Look ! If the filtration is done on paper, the paper is quickly transformed into a sort of parchment, that prevents any liquid from going through. And if it is done on a glass-sintered filter, the glass will be attacked by $$\ce{NaOH}$$. As a consequence, I am afraid there is no possibility of separating easily $$\ce{NaCl}$$ from $$\ce{NaOH}$$. The only really working process would be centrifugation, which requires an equipment that is not always available in all laboratories.