16:I[8216,["972","static/chunks/972-b28da0de92681928.js","47","static/chunks/47-a7f06e9eda1ac756.js","115","static/chunks/app/%5Bexam%5D/questions/%5Byear%5D/%5Bsubject%5D/%5Bchapter%5D/%5BquestionId%5D/page-7b6f0a12b9cc0206.js"],"BackButton"] 17:I[1553,["972","static/chunks/972-b28da0de92681928.js","47","static/chunks/47-a7f06e9eda1ac756.js","115","static/chunks/app/%5Bexam%5D/questions/%5Byear%5D/%5Bsubject%5D/%5Bchapter%5D/%5BquestionId%5D/page-7b6f0a12b9cc0206.js"],"QuestionViewer"] 15:T51b,{"@context":"https://schema.org","@type":"Quiz","name":"Mht Cet 2025 Liquid Solution PYQ with Solution","url":"https://pyq-test-series-platform-alsjdcxu2-sameers-projects-41c5a71e.vercel.app/mht-cet/questions/2025/chemistry/liquid-solution/meujcb4t","educationalLevel":"Entrance exam preparation","about":"Mht Cet / Chemistry / Liquid Solution","hasPart":{"@type":"Question","name":"Mht Cet 2025 Liquid Solution PYQ with Solution","text":"Calculate the percent dissociation of 0.02 m solution if its freezing point depression is 0.046 K . \\left[\\mathrm{K}_{\\mathrm{f}}\\right. for water \\left.=1.86 \\mathrm{~K} \\mathrm{~kg} \\mathrm{~mol}^{-1} ; \\mathrm{n}=2\\right]","eduQuestionType":"mcq","acceptedAnswer":{"@type":"Answer","text":"B"},"comment":{"@type":"Comment","text":"Given data: Molality, m = 0.02\\ \\text{m} Depression in freezing point, \\Delta T_f = 0.046\\ \\text{K} Cryoscopic constant, K_f = 1.86\\ \\mathrm{K\\,kg\\,mol^{-1}} Number of ions after dissociation, n = 2 Step 1: Write formula for depression in freezing point \\Delta T_f = i \\cdot K_f \\cdot m where i is the van't Hoff factor. Step 2: Calculate van't Hoff factor i i = \\frac{\\Delta T_f}{K_f \\cdot m} Substitute values: i = \\frac{0.046}{1.86 \\times 0.02} = \\frac{0.046}{0.0372} \\approx 1.24 Step 3: Relate..."}}}18:T4d5,

Given data:

Molality, $m = 0.02\ \text{m}$
Depression in freezing point, $\Delta T_f = 0.046\ \text{K}$
Cryoscopic constant, $K_f = 1.86\ \mathrm{K\,kg\,mol^{-1}}$
Nu

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