When sodium chloride (NaCl) dissolves in water, it dissociates into its constituent ions: Na\(^+\) and Cl\(^-\). When the student adds concentrated sodium hydroxide (NaOH) to the saturated NaCl solution, the OH\(^-\) ions from NaOH react with the Na\(^+\) ions to form sodium hydroxide in solution. This reaction effectively reduces the concentration of Na\(^+\) in the solution, shifting the equilibrium of the NaCl dissolution reaction to the right in an attempt to restore equilibrium by producing more Na\(^+\) and Cl\(^-\) ions from solid NaCl. As a result, if the NaCl solubility limit is exceeded due to changes in ion concentrations, a precipitate of solid NaCl may form.
Use the equation of sodium chloride dissolving in water to complete the activity.NaCl(s) ⇌ Na+ (aq) + Cl−(aq) A student prepares a saturated sodium chloride solution. The student adds concentrated sodium hydroxide (NaOH) to the solution until a precipitate forms. What is happening with the equilibrium? In three to five sentences, explain your answer.
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