Is it true that more potassium bromide can dissolve in distilled water than in a solution of potassium chloride? Im thinking maybe the common ion effect is present here?

I don't know the numbers but I'm inclined to think that what you have said is true. I'm not so sure that it has anything to do with the common ion effect, although there is a common ion, but that effect usually only comes into play with slightly soluble materials.

There has been some research that indicates in addition to ions, complexes form in the solution, in particular, a (KBr-KCl)(OH-), so it appears that there are more ions in solution. When crystalized, these complexes have a very useful light output when excited (a Laser).

When 25 mL of 0.24 mol/L CaCl2 is mixed with 45 mL of 1.5 mol/L AgNO3, a precipitate of AgCl forms because the Ksp of AgCl is 1.8 x 10^-10

Is this true or false?

After I responded to your post above, concerning the solubility of KCl in water vs NaCl solution, I took a shower. While in the shower I decided my answer might not be right and should be reconsidered. So scratch what I said, it may very well be true that more KCl can dissolve in a NaCl solution than in pure water. As I said before, I don't have any numbers to back up either answer.

Calculate mols and concns and determine if Ksp is exceeded.

mols CaCl2 = M x L = 0.24 M x 0.025 L = 0.006 and there are two Cl^- ions so that is 0.012 mols Cl^-.

mols AgNO3 = 1.5 M x 0.045 L = 0.0675 mols Ag^+.

(Ag^+) = mols/L = 0.0675/0.070 L = 0.964 M
Cl^-) = 0.012/0.070 = 0.171 M.

Kquotient=0.964*0.171 = a larger number than Ksp; theerefore, a ppt of AgCl will occur. Check my work.

Sure thing:P

Can you help me with one very last question?

In a saturated solution of silver nitrate the concentration of aluminum ion is 2.4 x 10^-8 mol/L. What is the Ksp of aluminum hydroxide?

I really don't even know where to start......

I thought I gave you the answer for that and you said you had worked it right!.

Al(OH)3 ==> Al^+3 + 3OH^-
Ksp = (Al^+3)(OH^-)^3
Al ion = 2.4 x 10^-8; therefore, OH^- = 3 x 2.4 x 10^-8= 7.2 x 10^-8
Ksp = (2.4 x 10^-8)(7.2 x 10^-8)^3 =9.0 x 10^-30

Im really sorry I got sidetracked:P This is the question I wanted to ask you

In a saturated solution of silver sulfite, the concentration of silver ion is 3.6 x 10^-4 mol/L. The Ksp of silver sulfite willl be what?

Sorry about that

Answered above.

Yes, it is true that more potassium bromide (KBr) can dissolve in distilled water compared to a solution of potassium chloride (KCl). The reason for this can be explained by the common ion effect.

The common ion effect occurs when two solutes with a common ion are dissolved in a solvent. In this case, both potassium bromide and potassium chloride contain the common ion, potassium (K+). When a solute with a common ion is dissolved in a solution, the presence of the common ion already in the solution reduces the solubility of the solute.

In the case of potassium bromide, when dissolved in distilled water, it does not encounter the common ion potassium from any other source. Therefore, the solubility of potassium bromide in distilled water is relatively higher.

However, when potassium bromide is dissolved in a solution of potassium chloride, the already present potassium ions from the potassium chloride reduce the solubility of the potassium bromide. This is because the excess potassium ions already in the solution create an unfavorable environment for additional potassium bromide to dissolve.

To further understand and quantify the common ion effect, you can compare the solubility products (Ksp) of potassium bromide and potassium chloride. The Ksp is a measure of the solubility of a compound. Comparing these values will provide you with a concrete understanding of the solubility difference.

In summary, more potassium bromide can dissolve in distilled water compared to a solution of potassium chloride due to the common ion effect caused by the presence of excess potassium ions in the solution.