200 mL of an aqueous solution contains 0.030 M concentrations of both Pb²⁺ and Ag⁺. If 100 mL of 6.0 × 10^-2 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The K_sp values for PbCl₂ and AgCl are 1.7 × 10^-5 and 1.8 × 10^-10.Hint: Remember that the solutions are being diluted and use the diluted concentrations.

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The Answer of 200 mL of an aqueous solution contains 0.030 M concentrations of both Pb²⁺ and Ag⁺. If 100 mL of 6.0 × 10^-2 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The K_sp values for PbCl₂ and AgCl are 1.7 × 10^-5 and 1.8 × 10^-10.Hint: Remember that the solutions are being diluted and use the diluted concentrations.

200 ML of an Aqueous Solution Contains 0