Question
Why do the concentrations of Pb 2+ and SO4 2- ions in a saturated solution of PbSO4 in contact with solid PbSO4 remain the same when the solution evaporates to half of its original volume?
it has to do with equilibrium.
it has to do with equilibrium.
Answers
PbSO4(s) ==> Pb^2+(aq) + SO4^2-(aq)
Ksp = (Pb^2+)(SO4^2-)
As the solvent evaporates, Ksp must stay the same; therefore, PbSO4 must come out of solution to keep the ion product the same.
Ksp = (Pb^2+)(SO4^2-)
As the solvent evaporates, Ksp must stay the same; therefore, PbSO4 must come out of solution to keep the ion product the same.
Related Questions
I have no idea how to solve this problem, please help me out.... thanks
a) A liter of a soluti...
Calculate the concentrations of all ions after 50.0 mL of a 0.100 M AgNO3 solution is mixed with 100...
What is the Ksp of Lead II Fluoride if the lead and fluoride ions have molecular concentrations of 4...
Solubility of Calcium Hydroxide
At some temperature, the solubility of Ca(OH)2 is 0.0880 g/100mL....