stuck. Will a precipitate form?

Question

The Ksp of silver Bromide is 4.1x10^(-13). Will a precipitate form if 25.0mL of .0345M silver nitrate solution is mixed with 25.0mL of 3.63x10^(-4)M sodium bromide solution?

I'm clueless on this?

Answer 1

Silver nitrate is very soluble in water.
Silver bromide is not.
So if you have too much bromide ion in water, the Ksp may put a limit on the silver & bromide ion that can stay in water. If there is more, you have a AgBr ppt.

So lets do the math:
Step 1. find the amount of silver g-ion in 25 mL of 0.0345 M AgNO3. To do this mult 0.025 L x .0345
Step 2. find the amount of bromide g-ion in 25 ml of 0.000363 M NaBr.
Step 3. Convert each to mole/liter by multiplying each by 20 (go from 50 mL to 1 L)
Step 4. With the amounts of each from step 3, do the Ksp test.
Is [Ag+][Br-] < Ksp
Yes- no ppt
No - ppt.

Answer 2

Remember the E values for the formation of silver bromide, those are related to the concentration of Ag+ and Cl-. If you are given the Ksp, then you need to see what the Eo values are for the formation of AgBr.

Answer 3

2 Ag+ +Br2- ->Ag2Br
Ksp=[Ag+][Br2-]=4.1x10^(-13)
Now we calculate Qsp t compare with Ksp
concetration will be different because the volume of the solution is now 50ml not 25 any more
Qsp=[Ag+][Br2-]=(0.0342/2)*(3.63x10^(-4)/2)=(please use your calculator)

Qsp>Ksp so there is more product -> Precipitates will form
otherwise, it will not form

I'm not too confident, but hope it works

Answer 4

yes the precipitate is silver bromide