Several reactions are carried out using AgBr, a cream-colored silver salt for which the value of the solubility product constant, Ksp, is 5.0 x 10-13 at 298 K.
a) Calculate the value of [Ag+] in 50.0 mL of a saturated solution of AgBr at 298 K.
b) A 50.0 mL sample of distilled water is added to the solution described in part (b), which is in a beaker with some solid AgBr at the bottom. The solution is stirred and equilibrium is re-established. Some solid AgBr remains in the beaker. Is the value of [Ag+] greater than, less than, or equal to the value you calculated in part
c) Calculate the minimum volume of distilled water, in liters, necessary to completely dissolves a 5.0 g sample of AgBr at 298 K.
d) A student mixes 10.0 mL of 1.5 x 10-4 M AgNO3 with 2.0 mL of 5.0 x 10-4 M NaBr and stirs the resulting mixture. What will the student observe?
Is this a practice problem to check your answers? If so show your work and I'll check for you. If not, please explain what you don't understand about the problem and I'll help you through it.
I don't understand how to set it up and get started on the problem and this is a problem that our teacher gave us for practice for the AP Chem exam
Here is how you do a part. That should get you started.
.........AgBr ==> Ag^+ + Br^-
I........solid.....0......0
C........solid.....x......x
E........solid.....x......x
Substitute the E line into the Ksp expression and solve for x = (Ag^+) = (Br^-)
My presumption is that the answer for a is to be (Ag^+) in mols/L and the concn is the same whether the volume is 50 or 500.
Knowing this you should be able to answer b.
c is the just the reverse question in a.
D is a common ion problem and the concn of AgBr is less in that solution.
Post your work if you get stuck.