SOLVED: A saturated solution of lead iodate in pure water has a lead ion concentration of 4.0x10^-5 mole per liter at 20°C.(a) Calculate the value for the solubility product constant of Pb(IO3)2 at 25°C.(b) Calculate the molar solubility of Pb(IO3)2 in a 0.10-molar Pb(NO3)2 solution at 25°C.(c) To 333 milliliters of a 0.120-molar Pb(NO3)2 solution, 667 milliliters of 0.435-molar KIO3 is added.Calculate the concentrations of Pb2 and IO3- in the solution at equilibrium at 25°C.
SOLVED: A saturated solution of lead iodate in pure water has a lea…
Nov 8, 2022
numerade.com
The solubility of lead(II) iodate in pure water is 0.76  g ·L^-1 at 25^∘ C. Calculate the value of Kxp for lead(II) iodate at 25^∘ C. Is the value of Ksp you calculated the same as that listed in Table 22.1? Suggest a possible reason for any discrepancy. | Numerade
The solubility of lead(II) iodate in pure water is 0.76  g ·L^-1 at 25^∘ …
2 months ago
numerade.com
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