Final answer:
To calculate the minimum mass of NaCl necessary to dissolve 0.010 mol AgCl in 100L solution, we use the solubility product constant (Ksp) of AgCl and the formation constant (Kf) of AgCl₂⁻ complex ion.
Step-by-step explanation:
Since the volume is constant, we can assume that the AgCl will completely dissociate into Ag⁺ and Cl⁻ ions in the solution. The Ksp of AgCl is 1.6 × 10^-10. We can use this information to calculate the concentration of Ag⁺ ions in the solution, which is equal to the solubility of AgCl in pure water at 25°C.
To calculate the concentration of Ag⁺ ions, we use the equation [Ag⁺][Cl⁻] = Ksp. Therefore, [Ag⁺] = sqrt(Ksp) = sqrt(1.6 × 10^-10) = 1.26 × 10^-5 M. Now, we can calculate the mass of NaCl required to provide the same concentration of Cl⁻ ions. Thus, [Cl⁻] = [NaCl] = 1.26 × 10^-5 M.
Using the formula moles = concentration × volume, we can calculate the moles of NaCl required: moles = 1.26 × 10^-5 M × 100 L = 1.26 × 10^-3 mol. Finally, using the molar mass of NaCl (58.44 g/mol), we can calculate the minimum mass of NaCl required: mass = moles × molar mass = 1.26 × 10^-3 mol × 58.44 g/mol = 0.0737 g.