using leChatlier's principle, which of following is more or less soluble in following solutions than in pure water. and explaination for each asked for. Compared to pure water are they less, more or same? thanks.

AgBr in 0.100M HBr

AgBr IN 0.100 m HNO3

Fe(Oh)2 in 0.100 M HCl

Fe(OH)2 in 0.100 M naoh

Le Chatlier's Principle says that when a system at equilibrium is disturbed it will shift so as to undo what we've done it it.

AgBr in 0.1 M HBr.
......AgBr ==> Ag^|Using the balanced chemical equation, calculate the equilibrium constant for this system.
AgBr(s) ==> Ag^+(aq) + Br^-(aq)
(Note AgBr is only slightly soluble)
HBr ==> H^+ + Br^-.
(Note that HBr is a strong acid; it ionizes completely.)
So the AgBr is slightly soluble, it has dissolved as much as it can. When you add extra Br^- to it, it tries to get rid of the added Br^-. It can do that only one way. By shifting the equilibrium to the left; i.e., some of the Ag^+ in solution combines with some of the Br^- to form solid AgBr (in other words the rxn shifts to the left) and AgBr becomes less soluble when HBr is added.
The others are done the same way.
Note that in Fe(OH)2 and HCl that the HCl reacts to form H2O so you are removing OH^- from the solution. I'll be happy to review your answers.

yes, the first one i understood. It was more so when AgBr in HNO3, in an acid where i don't see a common ion. with the first one i calculated solubility mathematically even though i didn't need to. My answers are:

less soluble, more soluble, more, and less

AgBr in HNO3 is no effect (or the same solubility).

You're right, there is no common ion and the only rxn that you need to consider is combination of H with Br. IF (and it isn't) HBr were a weak acid it would be more soluble but since HBr is a strong acid there is no driving force so solubility in HNO3 is the same as if no HNO3 were there.

Alright. It makes more sense to me now. Thank you!

To determine whether a compound is more or less soluble in a specific solution compared to pure water using LeChatelier's principle, we need to consider the effect of the added solution on the equilibrium of the dissolution reaction. Specifically, we assess the effect of the common ion or pH changes on the solubility of the compound.

1. AgBr in 0.100 M HBr:
When AgBr dissolves in water, it dissociates into Ag+ and Br- ions due to the polar nature of water molecules. In this case, when HBr is added to water, it also dissociates into H+ and Br- ions. Since HBr provides additional Br- ions, which is one of the ions already present in AgBr, LeChatelier's principle predicts that the equilibrium will shift leftward, decreasing the solubility of AgBr. Therefore, AgBr is expected to be less soluble in 0.100 M HBr than in pure water.

2. AgBr in 0.100 M HNO3:
HNO3 is a strong acid that produces H+ ions when dissolved in water. Since AgBr contains Ag+ ions, which can react with H+ ions to form Ag(I) salt, the increased H+ concentration from HNO3 will drive the equilibrium towards the formation of Ag(I) salt. This shift will cause the solubility of AgBr to decrease. Thus, AgBr is expected to be less soluble in 0.100 M HNO3 compared to pure water.

3. Fe(OH)2 in 0.100 M HCl:
Fe(OH)2 is a weak base that reacts with H+ ions from acids. In this case, when HCl is added to water, it dissociates into H+ and Cl- ions. The increased H+ concentration will react with Fe(OH)2, converting Fe(OH)2 into FeCl2 salt. As a result, the equilibrium will shift rightward, causing the solubility of Fe(OH)2 to increase. Therefore, Fe(OH)2 is expected to be more soluble in 0.100 M HCl than in pure water.

4. Fe(OH)2 in 0.100 M NaOH:
NaOH is a strong base that dissociates in water to form Na+ and OH- ions. When Fe(OH)2 is added to this solution, the OH- ions will react with Fe(II) ions to form Fe(OH)3, which has lower solubility than Fe(OH)2. Consequently, the equilibrium will shift leftward, reducing the solubility of Fe(OH)2. Thus, Fe(OH)2 is expected to be less soluble in 0.100 M NaOH compared to pure water.

In summary:
- AgBr is less soluble in 0.100 M HBr and 0.100 M HNO3 compared to pure water.
- Fe(OH)2 is more soluble in 0.100 M HCl and less soluble in 0.100 M NaOH compared to pure water.