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NaCl(s) ⇄ Na+(aq) + Cl–(aq)

A student is testing two clear liquids. One liquid is water that has been modified to have a basic pH. The other liquid is a sports drink that contains added electrolytes, including Na+(aq). How can the student use the equilibrium reaction of sodium chloride to determine which liquid is which? In three to five sentences, explain your answer.

The student can add a small amount of NaCl(s) to each liquid and observe any changes in the solution. If the solution with a basic pH reacts with the NaCl to produce Na+(aq) and Cl–(aq), it indicates that the liquid is water modified to have a basic pH. On the other hand, if the solution with the added electrolytes already contains Na+(aq) and Cl–(aq), there won't be any visible reaction, and it indicates that the liquid is the sports drink.

By using the equilibrium reaction of sodium chloride, the student can determine which liquid is which based on the presence of Na+(aq). Since the equilibrium reaction involves the dissociation of NaCl into Na+(aq) and Cl-(aq), the student may test both liquids using a conductivity tester or voltmeter. If the liquid conducts electricity or shows a higher conductivity reading, it indicates the presence of Na+(aq), which suggests it is the sports drink containing added electrolytes. On the other hand, if the liquid does not conduct electricity well or shows a lower conductivity reading, it suggests the absence of Na+(aq) and implies it is the basic water. Additionally, the student can also use litmus paper or pH test strips to determine the basicity or alkalinity of the solution, further confirming the identity of the water.

To determine which liquid is which, the student can perform a simple experiment using sodium chloride (NaCl) and the two clear liquids. Firstly, the student can add a small amount of NaCl to each liquid separately and observe any changes. If the liquid that has been modified to have a basic pH is present, it will react with the NaCl to produce a visible precipitate, indicating the presence of chlorine ions (Cl–(aq)). This is because the basic solution will make the equilibrium reaction shift to the left, resulting in the formation of solid NaCl. On the other hand, if the sports drink contains added electrolytes (including Na+(aq)), there won't be a visible precipitate formation as the equilibrium will favor the formation of Na+(aq) and Cl–(aq), keeping the ions dissolved in the liquid.