Would the solubility of AgBr(s) in a .10 M. KNO3 be smaller, larger of the same as the solubility of AgBr(s) in water. Wouldn't it be larger?

Yes, it would be larger. Do you know why? It's important that you know why.

No i don't think i'm entirly sure why its larger?

Read about the effect of ionic strength on solubility (the activity and the activity coefficient). The activity coefficient is a factor used to correct for non-ideal behavior of solutions. In connection with this, you will see reverence to the Debye-Huckel theory (or equation)(often written as the DHE for Debye-Huckel equation) and the extended Debye-Huckel equation. (often written as EDHE)

To determine whether the solubility of AgBr(s) in a 0.10 M KNO3 solution is smaller, larger, or the same as the solubility of AgBr(s) in water, we need to consider the effect of the KNO3 solution on the solubility of AgBr(s).

When AgBr(s) dissolves in water, it dissociates into Ag+ and Br- ions. This dissolution process is governed by the solubility product constant (Ksp) of AgBr. The greater the value of Ksp, the more soluble the compound.

Now, let's consider the effect of adding a 0.10 M KNO3 solution to AgBr(s). KNO3 is a strong electrolyte that dissociates into K+ and NO3- ions. When KNO3 dissociates, it increases the concentration of the NO3- ions in the solution.

The presence of NO3- ions in the solution has an important effect on the solubility of AgBr(s). NO3- ions can react with Ag+ ions to form a slightly soluble compound called AgNO3. This process is governed by its own solubility product constant (Ksp). The formation of AgNO3 consumes Ag+ ions, reducing the concentration of the Ag+ ions available for the dissolution of AgBr(s).

Therefore, the addition of a 0.10 M KNO3 solution reduces the concentration of Ag+ ions in the solution, which, in turn, decreases the solubility of AgBr(s). This means that the solubility of AgBr(s) in a 0.10 M KNO3 solution would be smaller than in pure water.

In summary, the solubility of AgBr(s) in a 0.10 M KNO3 solution would be smaller than its solubility in water due to the formation of AgNO3 which reduces the concentration of Ag+ ions available for the dissolution of AgBr(s).