This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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D. Step 1: Write the dissolution equilibrium for silver chloride (AgCl). When AgCl dissolves in water, it dissociates into silver ions (Ag^+) and chloride ions (Cl^-). AgCl(s) Ag^+(aq) + Cl^-(aq) Step 2: Define the solubility product expression (Ksp). The solubility product constant for AgCl is given by the product of the concentrations of its ions at equilibrium. If 's' represents the molar solubility of AgCl, then [Ag^+] = s and [Cl^-] = s. Ksp = [Ag^+][Cl^-] = (s)(s) = s^2 Step 3: Calculate the molar solubility (s) of AgCl. Given Ksp = 2.0 × 10^-10 mol^2dm^-6. s^2 = 2.0 × 10^-10 mol^2dm^-6 s = sqrt(2.0 × 10^-10) mol^2dm^-6 s = 1.4142 × 10^-5 mol dm^-3 Step 4: Determine the quantity of silver lost. The quantity of silver lost in the process refers to the concentration of Ag^+ ions that dissolve in the water. This concentration is equal to the molar solubility (s). Quantity of silver lost = [Ag^+] = s = 1.414 × 10^-5 mol dm^-3. The value matches option D. The final answer is D. Send me the next one 📸