How do you calculate Ksp if given molar solubility?

1 Answer
anor277
Jun 27, 2016

I wil give you an example with regard to #K_(sp)# of #"silver bromide"#.

Explanation:

Write the solubility expression:

#AgBr rightleftharpoons Ag^(+) + Br^-#

Now the solubility of #AgBr# under standard conditions is reported as #5.71xx10^-7# #mol*L^-1#.

Given the solubility, #[AgBr]=[Ag^+]=[Br^-]#

And #K_(sp)# is simply the equilibrium expression, #[Ag^+][Br^-]# #=# #(5.71xx10^-7)^2# #=# #??#

Related questions
See all questions in Equilibrium Constants
Impact of this question
2572 views around the world
You can reuse this answer
Creative Commons License