1)
Use equilibrium ion concentration to calculate Ksp.
The Pb2+ concentration in a saturated solution of lead bromide is measured and found to be 1.19×10-2 M. Use this information to calculate a Ksp value for lead bromide.
Ksp =___________
2)
Use solubility to calculate Ksp.
The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide.
Ksp =______________
1) Lead bromide dissolves in water to a small extent according to the equation
PbBr2 = Pb^2+ + 2Br-
The concentration of Pb2+ = 1.19*10^-2M
if the concentration of Pb2+ is x, then concentration of Br- is 2x,i.e., 2.38*10^-2M
therefore, Ksp = (Pb2+)(Br-)^2 = (1.19*10^-2)(2.38*10^-2)^2 = 6.74*10^-6
2) Fe(OH)2 dissolves in water to a small extent according to the equation
Fe(OH)2 = Fe^2+ + 2OH-
The concentration of Fe2+ = weight/mol.wt = 1.15*10^-3/89.86 = 1.28*10^-5 M
if the concentration of Fe2+ is x, then concentration of OH- is 2x i.e., 2.56*10^-5M
therefore, Ksp = (Fe2+)(OH-)^2 = (1.28*10^-5)(2.56*10^-5)^2 = 8.38*10^-15
1) Use equilibrium ion concentration to calculate Ksp. The Pb2+ concentration in a saturated solution of...
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