) Which of the following should dissolve the smallest amount of silver sulfide per liter, assuming no complex formation? A) 0.1 M HNO3
B) 0.1 M Na2S
C) 0.1 M AgNO3
D) 0.10 M NaNO3
E) pure water
You can calculate the value.
Ag2S ==> 2Ag^+ + S^-2
Ksp = (Ag^+)^2(S^-2)
Plug in Ksp and 0.1 for sulfide and calculate solubility.
Now do the same for Ksp and 0.1 for Ag^+ and calculate solubility. Which is smaller? (HNO3 you know isn't the one because HNO3 will dissolve all of the Ag2S, NaNO3 and pure water dissolve the usual amount of Ag2S (which you can calculate if you wish from Ksp.)) However, you know that EITHER B or C will be the smallest amount because both B and C contain a common ion which will shift the solubility equilibrium to the left, thus reducing the solubility of Ag2S.
Well, let's see here. We're looking for the option that would dissolve the smallest amount of silver sulfide per liter without forming any complexes.
Option A: 0.1 M HNO3. Nitric acid is a strong acid, but it doesn't have any specific affinity for silver sulfide, so it might not be the best choice.
Option B: 0.1 M Na2S. Ah, sodium sulfide, an interesting choice. It actually reacts with silver sulfide to form silver thiosulfate, so it would dissolve some of the silver sulfide. Looks like we can rule this one out.
Option C: 0.1 M AgNO3. Ah, silver nitrate, the classic silver compound. Since silver sulfide is insoluble, silver nitrate might not have a significant effect on its dissolution.
Option D: 0.10 M NaNO3. Sodium nitrate, a common salt. It doesn't have any particular reactivity towards silver sulfide, so it might not dissolve much.
Option E: Pure water. Hahaha, well, water is known as the "universal solvent," but it might not be very effective in this case. Silver sulfide isn't very soluble in pure water.
So, after some clownish analysis, I'd say the option that would dissolve the smallest amount of silver sulfide per liter without forming any complexes is probably option C: 0.1 M AgNO3.
To determine which of the given options will dissolve the smallest amount of silver sulfide per liter, we need to consider the solubility of silver sulfide and the reaction it undergoes with the different solutions.
The solubility of silver sulfide (Ag2S) is low in most aqueous solutions due to its low solubility product constant (Ksp). In pure water (option E), silver sulfide will only dissociate to a very small extent, resulting in a low solubility.
Let's analyze the other options:
A) 0.1 M HNO3: Nitric acid is a strong acid and will readily dissociate in water, but it does not react directly with silver sulfide. Therefore, it will not dissolve silver sulfide.
B) 0.1 M Na2S: Sodium sulfide (Na2S) is a strong base. In the presence of silver sulfide, it will react to form silver sulfide complexes, thus dissolving silver sulfide. This option will dissolve a significant amount of silver sulfide.
C) 0.1 M AgNO3: Silver nitrate is a soluble salt that dissociates into Ag+ and NO3- ions in water. When added to silver sulfide, it will result in the formation of silver ions (Ag+), which can then react with sulfide ions (S2-) from the silver sulfide to form a soluble silver sulfide complex. This option will dissolve a significant amount of silver sulfide.
D) 0.10 M NaNO3: Sodium nitrate (NaNO3) is also a soluble salt that will dissociate in water and does not directly react with silver sulfide. Therefore, it will not dissolve silver sulfide.
Based on the given options, the solution that should dissolve the smallest amount of silver sulfide per liter, assuming no complex formation, is Option A) 0.1 M HNO3.
To determine which of the given options would dissolve the smallest amount of silver sulfide per liter, we need to understand the solubility rules for these compounds.
Silver sulfide (Ag2S) generally has low solubility in water because it is an insoluble salt. However, it can dissolve in certain solutions based on the solubility of its ions.
Let's analyze each option:
A) 0.1 M HNO3: Nitric acid is a strong acid, but it does not contain any ions that could dissolve silver sulfide. Therefore, it would not dissolve silver sulfide.
B) 0.1 M Na2S: Sodium sulfide (Na2S) is a strong base that dissociates to form S2- ions. These sulfide ions can react with silver ions from Ag2S to form an insoluble silver sulfide precipitate. Therefore, Na2S can dissolve a certain amount of silver sulfide, making it a possible option.
C) 0.1 M AgNO3: Silver nitrate (AgNO3) is a strong electrolyte that dissociates to form Ag+ ions. These silver ions can react with sulfide ions from Ag2S, forming silver sulfide precipitate. Therefore, AgNO3 can dissolve a certain amount of silver sulfide, making it a possible option.
D) 0.10 M NaNO3: Sodium nitrate (NaNO3) is a strong electrolyte that dissociates into Na+ and NO3- ions. None of these ions can react with silver sulfide to form a precipitate. Therefore, NaNO3 cannot dissolve silver sulfide.
E) Pure water: Pure water does not contain any ions that can react with silver sulfide. Hence, it is unlikely to dissolve a significant amount of silver sulfide.
Therefore, based on the given options, both B) 0.1 M Na2S and C) 0.1 M AgNO3 have the potential to dissolve silver sulfide to some extent. However, it's difficult to determine which one would dissolve the smallest amount without further information or experimental data.