What mass of NaCl should be found in 0.51 L of a saturated solution of sodium chloride if the Ksp of NaCl is assumed to be 1.5 x 10-5?
3 answers
The problem with this problem is that NaCl does not have a Ksp; therefore, I don't know the meaning of a Ksp for NaCl of 1.5 x 10^-5.
sorry Ksp of PbCl2 is 1.6 x 10-5
PbCl2 ==> Pb^+2 + 2Cl^-
Ksp = (Pb)(Cl^-)^2 = 1.5 x 10^-5
If we let y = solubility of PbCl2, then y = (Pb^+2) and 2y = (Cl^-).
Substitute y and 2y in the Ksp expression, solve for y and that will be the solubility of PbCl2 in mols/L. Multiplying by molar mass will give you the grams/L and multiplying that by 0.51/1 will give you the grams in 0.51 L.
Ksp = (Pb)(Cl^-)^2 = 1.5 x 10^-5
If we let y = solubility of PbCl2, then y = (Pb^+2) and 2y = (Cl^-).
Substitute y and 2y in the Ksp expression, solve for y and that will be the solubility of PbCl2 in mols/L. Multiplying by molar mass will give you the grams/L and multiplying that by 0.51/1 will give you the grams in 0.51 L.
1 answer