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
Step 1: Determine the moles of chloride ions (Cl^-) from HCl. HCl dissociates completely in water: HCl(aq) H^+(aq) + Cl^-(aq) Given 0.2 mole of HCl, it will produce 0.2 mole of Cl^- ions. Step 2: Determine the moles of chloride ions (Cl^-) from BaCl_2. BaCl_2 dissociates completely in water: BaCl_2(aq) Ba^2+(aq) + 2Cl^-(aq) Given 0.2 mole of BaCl_2, it will produce 2 × 0.2 = 0.4 mole of Cl^- ions. Step 3: Calculate the total moles of chloride ions. Total moles of Cl^- = Moles from HCl + Moles from BaCl_2 Total moles of Cl^- = 0.2 mol + 0.4 mol = 0.6 mol Step 4: Convert the volume of the solution to liters. Given volume = 500 mL 500 mL = 500 × (1)/(1000) L = 0.500 L Step 5: Calculate the molarity of chloride ions. Molarity is defined as moles of solute per liter of solution. Molarity of Cl^- = Total moles of Cl^-Volume of solution in liters Molarity of Cl^- = 0.6 mol0.500 L = 1.2 M The molarity of the Cl^- ions is 1.2 M. This corresponds to option (c). The final answer is 1.2 M. Send me the next one 📸