An aesthetically pleasing, abstract representation of a chemistry concept, illustrating the interplay between different chemical substances. The image should feature symbolic pictorial depictions of silver chloride (AgCl), hydrochloric acid (HCl), sodium nitrate (NaNO3), zinc chloride (ZnCl2), and silver nitrate (AgNO3). It should incorporate these entities in a way to portray a sense of penetrating scientific inquiry, possibly illustrating contrasting solubility of these substances, but without any text.

Silver chloride, AgCl, would be least soluble in

A.1.0M HCl
B.1.0M NaNO3
C.1.0M ZnCl2
D.1.0M AgNO3

and why?
thx

This is the common ion effect.

AgCl(s) --> Ag^+(aq) + Cl^-(aq)
Ksp = (Ag^+)(Cl^-)
Adding extra Ag^+ from AgNO3 increases (Ag^+) and that shifts the equilibrium to the left (to fewer ions and more solid) and that makes it less soluble. HCl will do the same thing as will ZnCl2. NaNO3 is the only one (excluding the effect of activity versus concn) that will not affect the solubility. So AgNO3 gives you 1 mole Ag^+/L, HCl gives 1 mole Cl^-/L but ZnCl2 will give two moles ZnCl2/L; therefore, the ZnCl2 will make it less soluble than the others.

In which of the following would silver chloride be least soluble?

View Available Hint(s)for Part B
pure water
1 M NaBr
1 M NaCl

Well, well, well, look who's asking about solubility. Are you trying to make silver chloride disappear? Sneaky little chemist, I see. Anyway, let's get straight to it.

Out of these options, the least soluble choice for silver chloride, AgCl, would be C. 1.0M ZnCl2. Why, you ask? Because AgCl and ZnCl2 are both ionic compounds, and when you mix two ionic compounds together, they can compete for the same ions in solution. Since zinc chloride (ZnCl2) has more chloride ions (Cl-) than any of the other options, it will gobble them up like a hungry monster, leaving little to no chloride ions available for the silver chloride to dissolve.

So, in conclusion, if you want to keep that silver chloride intact, stay away from the ZnCl2 solution. It's like trying to find a parking spot during rush hour – it's just not going to happen. Good luck with your chemistry adventures!

To determine which solution would be least soluble for silver chloride (AgCl), we need to consider the solubility rules and the common ion effect.

The solubility rules state that most chloride salts are soluble, except for those of silver, lead, and mercury(I) ions.

In this case, we have AgCl, a silver chloride salt. When AgCl dissolves in water, it dissociates into silver ions (Ag+) and chloride ions (Cl-).

Let's analyze each option:

A. 1.0M HCl: HCl is a strong acid that fully dissociates into hydrogen ions (H+) and chloride ions (Cl-). Since we already have excess chloride ions present (from AgCl), the equilibrium will shift towards the left according to Le Chatelier's principle, making AgCl less soluble. So, option A would make AgCl less soluble.

B. 1.0M NaNO3: Sodium nitrate (NaNO3) does not contain chloride ions. It has nitrate ions (NO3-), which would not affect the solubility of AgCl. So, option B would make AgCl more soluble.

C. 1.0M ZnCl2: Zinc chloride (ZnCl2) contains chloride ions as well. Similar to option A, it would provide additional chloride ions, causing the equilibrium to shift towards the left, thus making AgCl less soluble. So, option C would make AgCl less soluble.

D. 1.0M AgNO3: Silver nitrate (AgNO3) contains silver ions (Ag+), which would increase the concentration of Ag+ ions in the solution. Since AgCl will dissociate into Ag+ ions, the presence of additional Ag+ ions from AgNO3 will further push the equilibrium to the right, making AgCl more soluble. So, option D would make AgCl more soluble.

Based on the analysis, the solution least likely to dissolve AgCl is option B, 1.0M NaNO3, because it does not contain any ions that would affect the solubility of AgCl.

To determine the solubility of silver chloride (AgCl) in the given solutions, we need to consider the common ion effect. The common ion effect occurs when a compound is dissolved in a solution that already contains one of its constituent ions.

The solubility of AgCl can be represented by the following dissociation equation:

AgCl(s) ⇌ Ag⁺(aq) + Cl⁻(aq)

Now, let's analyze each option:

A. 1.0M HCl: When HCl dissociates, it forms H⁺ and Cl⁻ ions. Since Cl⁻ is already present in the solution, it will increase the concentration of the chloride ions and shift the equilibrium to the left, decreasing the solubility of AgCl. Therefore, silver chloride would be least soluble in 1.0M HCl.

B. 1.0M NaNO3: Sodium nitrate (NaNO3) dissociates into Na⁺ and NO3⁻ ions. As there is no common ion with AgCl, the solubility of AgCl would not be affected. Therefore, this solution would not have any significant impact on the solubility of AgCl.

C. 1.0M ZnCl2: Zinc chloride (ZnCl2) dissociates into Zn²⁺ and 2Cl⁻ ions. Since Cl⁻ is already present in the solution, it will increase the concentration of the chloride ions and shift the equilibrium to the left, decreasing the solubility of AgCl. Therefore, silver chloride would be less soluble in 1.0M ZnCl2 compared to NaNO3.

D. 1.0M AgNO3: Silver nitrate (AgNO3) dissociates into Ag⁺ and NO3⁻ ions. As Ag⁺ is the common ion with AgCl, it will increase the concentration of Ag⁺ ions in the solution. This will shift the equilibrium to the right, causing more AgCl to dissolve. Therefore, silver chloride would be more soluble in 1.0M AgNO3 compared to the other solutions.

Based on the analysis above, the correct answer is A. 1.0M HCl, as the common chloride ion will reduce the solubility of AgCl by shifting the equilibrium to the left.