Answer:
When we add 12M HCl, reaction quotient Qsp becomes greater than Ksp of NaCl leading to precipitation
Explanation:
When sodium chloride is dissolved in water, the equilibrium dissolution process known as Ksp is set up as typified by the equation;
NaCl(s)------> Na^+(aq) + Cl^-(aq)
According to Le Chatelier's principle, this system will remain in equilibrium after the addition of the 1M HCl. This explains why there will not be any change in the system after adding this solution.
However, addition of 12 M HCl will significantly distort the equilibrium position since there is now more Cl^- ion in the system. The system now seeks to relieve this stress by recrystallizing more sodium chloride leading to the formation of a precipitate. Succinctly put, when we add the 12M HCl, the reaction quotient Qsp becomes greater than Ksp of NaCl leading to precipitation of NaCl crystals.
When we add 12-M (concentrated) H-C-I, reaction quo-ti-ent becomes high that leading to pre-ci-pi-ta-tion.
In the case when sodium chloride should be dissolved in water, the equilibrium diss-olu-tion process is developed as typified by the equation;
[tex]NaCl(s)\rightarrow Na^+(aq) + Cl^-(aq)[/tex]
Now as per the principle, this system will remain in equilibrium after the addition of the 1-M is done. But the addition of 12-M will significantly distort the equilibrium position since there is now more [tex]Cl^-[/tex] ion in the system.
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