what would you observe when HCL gas is passed into the saturated soluction of NACL
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We will observe the formation of pure NaCl solid pricipitation from the solution.The principle behind this phenomenon is LeChatelier's principle.
When you have a saturated NaCl solution you have the equilibrium:
NaCl(s) <=> Na+(aq) + Cl-(aq)
When you add more Cl- to the already saturated solution, the equilibrium must shift to the left to undo the change which results in forming more NaCl(s). When your solution contains no solid phase and all of the NaCl is present as ions in solution then you are able to produce very pure NaCl(s) by bubbling HCl(g) into the saturated solution of NaCl.
When you have a saturated NaCl solution you have the equilibrium:
NaCl(s) <=> Na+(aq) + Cl-(aq)
When you add more Cl- to the already saturated solution, the equilibrium must shift to the left to undo the change which results in forming more NaCl(s). When your solution contains no solid phase and all of the NaCl is present as ions in solution then you are able to produce very pure NaCl(s) by bubbling HCl(g) into the saturated solution of NaCl.
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Answer:
when hcl gas is passed through a saturated nacl solution, the number of cl-1 ions increases. The increased number of cl-1 interact with na+1 ions to form crystallised nacl. Thus, the solubility of nacl decreases and it is recovered in crystalline form. This phenomenon is called common ion effect.
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