If you have the molar solubility of PbBr2 is 1.0x10^-2, whatis the Ksp? Could so

Question

If you have the molar solubility of PbBr2 is 1.0x10^-2, whatis the Ksp?
Could someone just explain to me the steps involved in thisproblem? I know that 1 mol of Pb is produced, along with 2 mols ofBr. So, K(sp)= (Pb)(Br)^2. If you plug in the molar solubility(1.0x10^-2) wouldn't you get: Ksp = (1.0x10^-2)[(1.0x10^-2)^2] which would be 1.0x10^-6?    If you have the molar solubility of PbBr2 is 1.0x10^-2, whatis the Ksp?
Could someone just explain to me the steps involved in thisproblem? I know that 1 mol of Pb is produced, along with 2 mols ofBr. So, K(sp)= (Pb)(Br)^2. If you plug in the molar solubility(1.0x10^-2) wouldn't you get: Ksp = (1.0x10^-2)[(1.0x10^-2)^2] which would be 1.0x10^-6?   

Explanation / Answer

PbBr2 Pb+2 + 2Br- x               x        2x Ksp = [Pb+2][Br-]2 If we consider the molar solubility of PbBr2as x mol/L Then Ksp = x * (2x)2                 = 4x3 The molar solubility of PbBr2 is 1.0 *10-2 Ksp = 4(1.0*10-2)3          = 4.0*10-6          = 4.0*10-6

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