the solubility of AgCl in HCl is
a. low, as Cl- ions cause an equilibrium shift towards the solid form
b. low, as Ag+ has already reacted with Cl-
c. high, as HCl readily ionizes
d. high, as AgCl can then form
e. high, as H2 forms, then escapes
(a) The scant amount of Ag+ is in solution will just combine with the added Cl- to form more AgCl solid.
a is the correct answer. Think Le Charelier's Principle. The solubility is
AgCl(s) ==> Ag^+(aq) + Cl^-(aq)
When HCl is added, it increase (Cl^-) on the right so the reaction shifts to the left making some AgCl ppt and the Ag^+ is decreased. Therefore, the solubility is decreased.
Well, I guess AgCl doesn't like hanging out in HCl solution. It's like that one friend who doesn't enjoy crowded places and just wants some peace and quiet. So, the solubility of AgCl in HCl is low because those pesky Cl- ions cause an equilibrium shift towards the solid form. It's like they're saying, "Hey AgCl, we're crashing your party whether you like it or not!" Poor AgCl just wants to be left alone in its solid state.
To summarize, the solubility of AgCl in HCl is low because the increase in Cl- ions caused by the addition of HCl shifts the equilibrium towards the solid form of AgCl. This decreased the concentration of Ag+ ions in solution and thus decreases the solubility of AgCl. Therefore, option (a) is the correct answer.
To determine the solubility of AgCl in HCl, we need to consider the chemical equilibrium reaction:
AgCl (s) ⇌ Ag+ (aq) + Cl- (aq)
In this reaction, AgCl is in a solid state, and when it comes into contact with water, it dissociates into Ag+ and Cl- ions, which are in an aqueous state.
Now, let's analyze the given options:
a. Low, as Cl- ions cause an equilibrium shift towards the solid form.
This option is correct. According to Le Châtelier's principle, when more Cl- ions are added to the reaction, it will cause a shift in equilibrium towards more AgCl(s) forming. Therefore, the solubility of AgCl will be low.
b. Low, as Ag+ has already reacted with Cl-.
This option is incorrect. Ag+ ions do not react with Cl- ions in the presence of HCl. The reaction only occurs when AgCl is in contact with water, not HCl.
c. High, as HCl readily ionizes.
This option is incorrect. The ionization of HCl does not directly affect the solubility of AgCl. The solubility depends on the equilibrium between AgCl(s) and Ag+ (aq) + Cl- (aq).
d. High, as AgCl can then form.
This option is incorrect. AgCl is already present in the reaction, and it forms when Ag+ and Cl- ions combine. The option does not provide a valid explanation for the solubility of AgCl.
e. High, as H2 forms, then escapes.
This option is incorrect. The formation and escape of H2 gas do not directly affect the solubility of AgCl. The solubility depends on the equilibrium between AgCl and its dissociation into Ag+ and Cl- ions.
Therefore, option a. Low, as Cl- ions cause an equilibrium shift towards the solid form, is the correct answer based on Le Châtelier's principle.