When the student adds concentrated sodium hydroxide (NaOH) to the saturated sodium chloride solution, the hydroxide ions (OH⁻) from the NaOH will react with the sodium ions (Na⁺) present in the solution to potentially form sodium hydroxide (NaOH) and remove Na⁺ from the solution. According to Le Chatelier's principle, removing reactants from one side of the equilibrium (in this case, Na⁺) will shift the equilibrium position to the left to compensate for the change, favoring the formation of solid NaCl (s) from its aqueous ions. As a result, the precipitation of NaCl occurs as the concentration of Na⁺ decreases, leading to more solid NaCl forming from the dissolved ions. Thus, the equilibrium shifts to the left, resulting in the formation of a precipitate.
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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