Suppose you had an unknown solution that contained either dissolved NaCL, or NaNO3. You added AgNO3 to the unknown solution and observed that no solid forms. What can be concluded about the unknown solution? (use the solubility rules
See your other post above.
To determine what can be concluded about the unknown solution, we need to consider the solubility rules for sodium chloride (NaCl) and sodium nitrate (NaNO3) when mixed with silver nitrate (AgNO3). The solubility rules allow us to predict whether a solid will form when two solutions are mixed.
First, let's examine the solubility rules for NaCl and AgNO3:
1. All nitrates (NO3-) are soluble.
2. Most sodium (Na+) compounds are soluble.
3. Silver (Ag+) compounds are generally insoluble, except for nitrates (AgNO3) and acetates (AgC2H3O2).
Based on these solubility rules, we can deduce the following:
1. NaNO3 (sodium nitrate) is soluble in water; therefore, when mixed with AgNO3, no reaction will occur, and no solid will form.
2. NaCl (sodium chloride) is also soluble in water. However, when mixed with AgNO3, a reaction will occur since silver chloride (AgCl) is insoluble in water.
Considering that no solid forms when AgNO3 is added to the unknown solution, we can conclude that the unknown solution likely contains dissolved sodium nitrate (NaNO3) rather than sodium chloride (NaCl).