Ksp = [Hg₂²⁺][Cl⁻]² = 1.3 × 10⁻¹⁸ [Cl⁻] = √(Ksp / [Hg₂²⁺]) = √(1.3×10⁻¹⁸ / 0.01) = √(1.3×10⁻¹⁶) = 1.14 × 10⁻⁸ M
The worksheet will ask you to calculate the exact concentration of the added ion ( Ag+Ag raised to the positive power ) required to initiate the precipitation of each compound. Rearranged: Calculation for : fractional precipitation pogil answer key
If your salt produces multiple ions (like ), remember to square the ion concentration in your Kspcap K sub s p end-sub expression: Ksp = [Hg₂²⁺][Cl⁻]² = 1