Add AgNO₃ solution to both unlabeled flasks: based on solubility rules, you can predict that when you add AgNO₃ to the NaCl solution, you will obtain AgCl precipitate, while no precipitate will be formed from the NaClO₃ solution.
<u>3. Relevant solubility rules for the problem.</u>
Although most salts containing Cl⁻ are soluble, AgCl is a remarkable exception and is insoluble.
All chlorates are soluble, so AgClO₃ is soluble.
Salts containing nitrate ion (NO₃⁻) are generally soluble and NaNO₃ is not an exception to this rule. In fact, NaNO₃ is very well known to be soluble.
Hence, when you add AgNO₃ to the NaCl solution the AgCl formed will precipitate, and when you add the same salt (AgNO₃) to the AgClO₃ solution both formed salts AgClO₃ and NaNO₃ are soluble.
Then, the precipiate will permit to conclude which flask contains AgCl.
Line 1: straight horizontal line Line 2: straight line at a slope Line 3: exponential growth curve Line 4: the topmost curve (the one that initially increases but then starts levels out)
