Chemistry question about solubility products and #K_(sp)#?
A solution contains #1.0 * 10^-4# M #Pb^(2+)# and #2.0 * 10^(-3)# M #Sr^(2+)# . If a source of #SO_4^(2-)# is added to this solution, will #PbSO_4# (#K_(sp)# = #1.8 * 10^(-8)# ) or #SrSO_4# (#K_(sp)# = #3.4 * 10^(-7)# ) precipitate first? Specify the concentration of #SO_4^(2-)# necessary to begin precipitation of each salt.
A solution contains
1 Answer
See Below
Explanation:
Oh,
We just treat them individually to start. I'm going to start with
I - +0.0001 0
C +s +s
E (0.0001+s) +s
Quadratic Equation: s = 0.0000932M
This tells you the concentration of
I - +0.002 0
C +s +s
E (0.002+s) +s
Quadratic Equation: s = 0.000159M
This tells you the concentration of
This means