Shown above is information about the dissolution of AgCl(s) in water at 298 K. In a chemistry lab a student wants to determine the value of s, the molar solubility of AgCl(s), by measuring [Ag+] in a saturated solution prepared by mixing excess AgCl and distilled water. How would the results of the experiment be altered if the student mixed excess AgCl with tap water (in which [Cl-]=0.010 M) instead of distilled water and the student did not account for the Cl- in the tap water?
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Shown above is information about the dissolution of AgCl(s) in water at 298 K. In a chemistry lab a...
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