When the student adds concentrated sodium hydroxide (NaOH) to the saturated sodium chloride (NaCl) solution, a precipitate forms due to the reaction between Na⁺ ions from the dissolved sodium chloride and OH⁻ ions from the sodium hydroxide. This leads to the formation of sodium hydroxide, which can precipitate out in the form of solid sodium chloride, effectively removing Na⁺ ions from the aqueous solution. According to Le Chatelier's principle, the removal of Na⁺ ions shifts the equilibrium of the dissolution reaction (NaCl(s) ⇌ Na⁺(aq) + Cl⁻(aq)) to the right, favoring the dissolution of more solid NaCl until saturation is re-established, until there is not enough NaCl to keep dissolving. As a result, the equilibrium shifts to maintain balance in response to the change in concentrations.
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
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