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?
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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?
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.
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......
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
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
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.
3 answers