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
Welcome back AUDREY — missed you this week. Here's the solution to question 6. Step 1: Calculate the molar mass of CaCl_2. The atomic mass of Ca is 40 and Cl is 35.5. Molar mass of CaCl_2 = 40 + (2 × 35.5) = 40 + 71 = 111 g/mol Step 2: Calculate the number of moles of CaCl_2. Given mass of CaCl_2 = 2.22 g. Moles of CaCl_2 = MassMolar mass = 2.22 g111 g/mol = 0.02 mol Step 3: Determine the moles of chloride ions (Cl^-). One mole of CaCl_2 dissociates into one mole of Ca^2+ and two moles of Cl^-. CaCl_2 (aq) → Ca^2+(aq) + 2Cl^-(aq) So, moles of Cl^- = 2 × moles of CaCl_2 = 2 × 0.02 mol = 0.04 mol Step 4: Convert the volume of water to dm^3. Given volume of water = 100 cm^3. Volume in dm^3 = 100 cm^31000 cm^3/dm^3 = 0.1 dm^3 Step 5: Calculate the concentration of chloride ions. Concentration = Moles of Cl^-Volume of solution in dm^3 = 0.04 mol0.1 dm^3 = 0.4 mol/dm^3 The concentration of chloride ions is 0.4 mol/dm^3$. Send me the next one 📸