Practice question

Given: What is the osmotic pressure of a solution containing 1.11 g of CaCl₂ in 300 mL of water at 27°C, assuming complete dissociation? ( R = 0.0821 L atm/mol K, Molar mass of CaCl₂ = 111 g/mol, i = 3 ) These values define the system as per NCERT data. Formula: Moles of CaCl₂ = 1.11/111 = 0.01 mol. This is standard NCERT relation. Substitution & Calculation: Molarity = 0.01/0.3 = 0.0333 M . Pi = i · C · R · T = 3 × 0.0333 × 0.0821 × 300 = 2.46 atm . Result: The computed value matches expected outcome and confirms correct choice as per NCERT.