I don't understand how to solve this. Please help!
At equilibrium:
PbF2 <----> Pb2+ + 2 F-
s 2s
Ksp = [Pb2+][F-]^2
3.3*10^-8=(s)*(2s)^2
3.3*10^-8= 4(s)^3
s = 2.021*10^-3 M
Answer: 2.02*10^-3 M
I don't understand how to solve this. Please help! Calculate the molar solubility of PbF2 in...
Calculate the molar solubility of PbF2 in water. The Ksp for PbF2 is 3.6 x 10-8. (Ignore the reaction of the F- ion with water.)
show work please
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Use the given molar solubilities in pure water to calculate the Ksp for each compound. PbF2 molar solubility of 5.63 x 10-3 M. Can you please show me the steps to show this problem? I know what the answer to the problem is but I can't get the steps right to come to the right answer.
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1. a. What is the molar solubility of Ag2SO4 (Ksp = 1.2 x 109) in water? b. How do you expect the solubility to change if the Ag2SO4 were in a 0.10M AgNO3 solution (increase, decrease, stay the same)? Why? C. Calculate the molar solubility of Ag2SO4 in 0.10M AgNO3. d. How do you expect the solubility to change if the Ag2SO4 were in a 0.10M HCl solution (increase, decrease, stay the same)? Why? Your explanation should...
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Calculate the molar solubility of Cu2SO3 (Ksp 8.1 x 1016) a) in water b) in 0.10 M CUNO3(aq) solution Will PBF2(s) form when 100 mL of 0.010 M Pb(C2H3O2)2(aq) is mixed with 100 mL of 0.0020 M NH4F(aq)? Explain (show all your work). (Ksp( PbF2)= 4.1 x 10
Calculating Molar Solubility:
(Please show all work! will upvote.)
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