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.
ScanSolve AI Answer
C. 1.69 × 10^-10 mol_2 dm^-6 Step 1: Write the dissociation equation for silver chloride (AgCl). Silver chloride is a sparingly soluble ionic compound that dissociates in water as follows: AgCl(s) Ag^+(aq) + Cl^-(aq) Step 2: Relate the concentration of the saturated solution to the solubility (s). The concentration of a saturated solution of AgCl is given as 1.30 × 10^-5 mol dm^-3. This value represents the molar solubility (s) of AgCl. From the dissociation equation, for every mole of AgCl that dissolves, one mole of Ag^+ ions and one mole of Cl^- ions are produced. Therefore, the concentration of Ag^+ ions is [Ag^+] = s = 1.30 × 10^-5 mol dm^-3. And the concentration of Cl^- ions is [Cl^-] = s = 1.30 × 10^-5 mol dm^-3. Step 3: Write the expression for the solubility product constant (K_sp). For the dissociation of AgCl, the solubility product expression is: K_sp = [Ag^+][Cl^-] Step 4: Substitute the solubility (s) into the K_sp expression and calculate the value. K_sp = (s)(s) = s^2 K_sp = (1.30 × 10^-5 mol dm^-3)^2 K_sp = (1.30)^2 × (10^-5)^2 mol^2 dm^-6 K_sp = 1.69 × 10^-10 mol^2 dm^-6 The calculated solubility product matches option C. The final answer is 1.69 × 10^-10 mol_2 dm^-6.