{"id":163035,"date":"2026-05-03T04:36:56","date_gmt":"2026-05-03T04:36:56","guid":{"rendered":"https:\/\/news.gyankatta.org\/?p=163035"},"modified":"2026-05-03T05:27:56","modified_gmt":"2026-05-03T05:27:56","slug":"class-12-chemistry-solutions-advanced-challenge-asset-pro-max","status":"publish","type":"post","link":"https:\/\/news.gyankatta.org\/?p=163035","title":{"rendered":"Class 12 Chemistry: Solutions &#8211; Advanced Challenge (ASSET Pro Max)"},"content":{"rendered":"\n<pre class=\"wp-block-code\"><code>\n\n<\/code><\/pre>\n\n\n\n<figure class=\"wp-block-image size-large\"><img decoding=\"async\" src=\"https:\/\/manishchandra.org\/p7\/cl12ChemSolutionsporster.png\" alt=\"\"\/><\/figure>\n\n\n\n<pre class=\"wp-block-code\"><code><\/code><\/pre>\n\n\n\n<div class=\"asset-pro-max-exam\">\n    <h2>Class 12 Chemistry: Solutions &#8211; Advanced Challenge (ASSET Pro Max)<\/h2>\n    <hr>\n\n    <!-- Question 1 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q1.<\/strong> A student observes that a mixture of Chloroform and Acetone becomes noticeably warm during the mixing process. Which of the following best explains the molecular behavior and the resulting vapor pressure of this solution?<\/p>\n        <ul>\n            <li>(A) The mixture shows a positive deviation from Raoult\u2019s Law because the new interactions are weaker than the pure component interactions.<\/li>\n            <li>(B) The mixture shows a negative deviation from Raoult\u2019s Law because hydrogen bonding occurs between the different molecules, lowering the total vapor pressure.<\/li>\n            <li>(C) The vapor pressure increases linearly with the mole fraction because the enthalpy of mixing is zero in this specific case.<\/li>\n            <li>(D) The boiling point of the mixture will be lower than that of both pure components due to the exothermic nature of the process.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 2 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q2.<\/strong> Why is the molarity of a solution considered an unreliable unit for experiments conducted across a wide range of temperatures, whereas molality remains consistent?<\/p>\n        <ul>\n            <li>(A) Molarity depends on the mass of the solvent, which can fluctuate due to evaporation at higher temperatures.<\/li>\n            <li>(B) Molarity is defined by the volume of the solution, which expands or contracts with temperature changes, altering the concentration value.<\/li>\n            <li>(C) Molality is a ratio of moles to the total volume of the solution, making it inherently more stable than mass-based units.<\/li>\n            <li>(D) The number of moles of solute actually increases at higher temperatures, but this effect is mathematically cancelled out in molality calculations.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 3 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q3.<\/strong> Consider three 0.1 m aqueous solutions: Glucose, Sodium Chloride, and Aluminium Sulfate. Which statement accurately compares their freezing points?<\/p>\n        <ul>\n            <li>(A) All three solutions will freeze at exactly the same temperature because they have the same molality.<\/li>\n            <li>(B) Glucose will have the lowest freezing point because it has the largest molecular weight among the three solutes.<\/li>\n            <li>(C) Aluminium Sulfate will have the lowest freezing point because it dissociates into the highest number of particles per formula unit.<\/li>\n            <li>(D) Sodium Chloride will have a lower freezing point than Aluminium Sulfate because the smaller size of its ions allows for faster freezing.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 4 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q4.<\/strong> In a scuba diving scenario, &#8216;the bends&#8217; is a painful condition caused by nitrogen bubbles forming in the blood. How does Henry\u2019s Law explain the prevention of this condition using Heliox (Helium-Oxygen mixture)?<\/p>\n        <ul>\n            <li>(A) Helium has a higher Henry\u2019s Law constant (K<sub>H<\/sub>) than Nitrogen, meaning it is less soluble in blood at high pressures.<\/li>\n            <li>(B) Helium is more soluble than Nitrogen at high pressures, ensuring that no gas escapes the blood during rapid ascent.<\/li>\n            <li>(C) The pressure of Helium is independent of the depth of the diver, preventing any changes in gas concentration in the tissues.<\/li>\n            <li>(D) Helium reacts chemically with hemoglobin to prevent other gases from dissolving in the plasma under extreme pressure.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 5 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q5.<\/strong> An azeotropic mixture of Ethanol and Water (95.4% ethanol) cannot be separated further by simple fractional distillation. This is primarily because:<\/p>\n        <ul>\n            <li>(A) The boiling points of the two pure components have become identical due to the high concentration of ethanol.<\/li>\n            <li>(B) The composition of the liquid phase is identical to the composition of the vapor phase at this specific concentration.<\/li>\n            <li>(C) Ethanol and Water form a solid complex at this ratio, which prevents the liquid from evaporating at all.<\/li>\n            <li>(D) The mixture shows a large negative deviation from Raoult&#8217;s Law, making the vapor pressure extremely low.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 6 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q6.<\/strong> If a non-volatile solute undergoes 80% dissociation in an aqueous solution, how does this specifically impact the calculated Osmotic Pressure compared to a non-electrolyte?<\/p>\n        <ul>\n            <li>(A) The osmotic pressure will be exactly double because dissociation always implies a two-fold increase in particle count.<\/li>\n            <li>(B) The osmotic pressure will be significantly higher than calculated for a non-electrolyte, as the Van&#8217;t Hoff factor (i) will be greater than 1.<\/li>\n            <li>(C) The osmotic pressure will decrease because the total volume of the solution increases when ions move apart.<\/li>\n            <li>(D) There will be no change in osmotic pressure because the total mass of the solute remains the same regardless of dissociation.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 7 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q7.<\/strong> Which of the following conditions must be met for a solution to be considered &#8216;Ideal&#8217; across the entire range of concentrations?<\/p>\n        <ul>\n            <li>(A) The heat of mixing must be negative to ensure that the molecules are strongly attracted to one another.<\/li>\n            <li>(B) The total volume of the solution must be exactly equal to the sum of the volumes of the two pure components.<\/li>\n            <li>(C) The solute must be significantly more volatile than the solvent to ensure rapid equilibration in the vapor phase.<\/li>\n            <li>(D) The mixture must form a maximum-boiling azeotrope to stabilize the vapor pressure against external fluctuations.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 8 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q8.<\/strong> When salt is spread on icy roads in cold climates, the ice melts. What is the underlying physical chemistry principle behind this practical application?<\/p>\n        <ul>\n            <li>(A) The salt reacts exothermically with the ice, generating enough heat to melt the surrounding frozen water.<\/li>\n            <li>(B) The addition of a non-volatile solute lowers the freezing point of water below the ambient temperature, causing the ice to liquefy.<\/li>\n            <li>(C) The salt particles act as abrasives that physically break the crystal lattice of the ice through friction.<\/li>\n            <li>(D) The salt increases the vapor pressure of the ice, causing it to sublime directly into gas without passing through the liquid phase.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 9 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q9.<\/strong> In the measurement of molar mass using colligative properties, why is Osmotic Pressure preferred for biological polymers like proteins over elevation of boiling point?<\/p>\n        <ul>\n            <li>(A) Proteins are highly volatile and would evaporate before the boiling point elevation could be accurately measured.<\/li>\n            <li>(B) The magnitude of osmotic pressure is much larger and easier to measure accurately for dilute solutions of high-mass molecules.<\/li>\n            <li>(C) Boiling point elevation requires a vacuum, which would cause the protein structure to collapse and denature.<\/li>\n            <li>(D) Osmotic pressure is the only colligative property that does not depend on the number of particles in the solution.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 10 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q10.<\/strong> How does the solubility of a solid solute in a liquid solvent typically change with an increase in temperature if the dissolution process is endothermic?<\/p>\n        <ul>\n            <li>(A) Solubility decreases as the system attempts to release the excess heat provided by the external environment.<\/li>\n            <li>(B) Solubility remains constant because the enthalpy of solution only affects the rate of dissolving, not the final equilibrium.<\/li>\n            <li>(C) Solubility increases because the addition of heat shifts the equilibrium toward the dissolved state to consume the energy.<\/li>\n            <li>(D) Solubility becomes zero at the boiling point because the solvent molecules move too fast to capture the solute particles.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 11 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q11.<\/strong> A solution of Benzoic acid in Benzene shows a molar mass that is nearly double its theoretical value. What molecular phenomenon explains this observation?<\/p>\n        <ul>\n            <li>(A) The Benzoic acid molecules are undergoing complete dissociation into ions within the non-polar benzene solvent.<\/li>\n            <li>(B) The Benzoic acid molecules are forming dimers through hydrogen bonding, effectively halving the number of individual particles.<\/li>\n            <li>(C) The Benzene solvent is reacting with the acid to form a heavy complex that precipitates out of the solution.<\/li>\n            <li>(D) The acid is behaving as a volatile solute, increasing the total vapor pressure beyond the predicted Raoult&#8217;s Law value.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 12 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q12.<\/strong> What occurs during the process of Reverse Osmosis when a pressure greater than the osmotic pressure is applied to the concentrated side of a solution?<\/p>\n        <ul>\n            <li>(A) Solute particles are forced through the membrane into the pure solvent side, leaving a diluted solution behind.<\/li>\n            <li>(B) Solvent molecules move from the region of higher solute concentration to the region of lower solute concentration.<\/li>\n            <li>(C) The semi-permeable membrane dissolves under high pressure, allowing both solute and solvent to mix freely.<\/li>\n            <li>(D) The temperature of the system rises until the osmotic pressure matches the applied external pressure.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 13 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q13.<\/strong> Which statement best describes the behavior of a &#8216;Minimum Boiling Azeotrope&#8217;?<\/p>\n        <ul>\n            <li>(A) It occurs in solutions that show a large negative deviation from Raoult\u2019s Law, resulting in a very high boiling point.<\/li>\n            <li>(B) It occurs in solutions that show a large positive deviation from Raoult\u2019s Law, resulting in a vapor pressure higher than pure components.<\/li>\n            <li>(C) It is a mixture that can be easily separated into pure components using a simple single-stage distillation flask.<\/li>\n            <li>(D) It only forms when the two liquids have identical molecular weights and identical intermolecular forces.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 14 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q14.<\/strong> If two solutions are isotonic, which of the following properties must they share at the same temperature?<\/p>\n        <ul>\n            <li>(A) They must have the same molar concentration of particles, resulting in identical osmotic pressures.<\/li>\n            <li>(B) They must contain the same mass of solute per liter of solvent, regardless of the solute&#8217;s molar mass.<\/li>\n            <li>(C) They must have the same boiling point elevation, even if one is aqueous and the other is an organic solution.<\/li>\n            <li>(D) They must have identical chemical identities and perform the same biological functions within a cell.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 15 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q15.<\/strong> A sample of water is contaminated with trace amounts of a heavy metal. Why is &#8216;Parts Per Million&#8217; (ppm) used instead of Molarity to report this concentration?<\/p>\n        <ul>\n            <li>(A) Ppm provides a much larger numerical value that is easier to record and interpret for extremely dilute concentrations.<\/li>\n            <li>(B) Molarity cannot be calculated for heavy metals because they do not have a defined molar mass in liquid form.<\/li>\n            <li>(C) Ppm is a volume-to-volume ratio that remains constant even if the density of the water changes significantly.<\/li>\n            <li>(D) Using Molarity would require knowing the exact volume of the entire ocean or water body being tested.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 16 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q16.<\/strong> According to Raoult&#8217;s Law, what happens to the relative lowering of vapor pressure when the mole fraction of a non-volatile solute is doubled?<\/p>\n        <ul>\n            <li>(A) The relative lowering of vapor pressure remains unchanged because it only depends on the nature of the solvent.<\/li>\n            <li>(B) The relative lowering of vapor pressure is doubled, as it is directly proportional to the mole fraction of the solute.<\/li>\n            <li>(C) The total vapor pressure of the solution doubles, making the liquid much more volatile than the pure solvent.<\/li>\n            <li>(D) The relative lowering of vapor pressure is halved because the solvent molecules now have more surface area to escape.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 17 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q17.<\/strong> How does the addition of a non-volatile solute affect the boiling point and vapor pressure of a solvent simultaneously?<\/p>\n        <ul>\n            <li>(A) It increases the vapor pressure and increases the boiling point by providing more energy to the system.<\/li>\n            <li>(B) It decreases the vapor pressure and increases the boiling point because more heat is needed to reach atmospheric pressure.<\/li>\n            <li>(C) It increases the vapor pressure and decreases the boiling point by disrupting the solvent-solvent attractions.<\/li>\n            <li>(D) It decreases both the vapor pressure and the boiling point because the solute particles act as cooling agents.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 18 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q18.<\/strong> What is the theoretical Van&#8217;t Hoff factor (i) for a dilute solution of Potassium Ferrocyanide, K<sub>4<\/sub>[Fe(CN)<sub>6<\/sub>], assuming complete dissociation?<\/p>\n        <ul>\n            <li>(A) i = 1, because the complex ion remains intact as a single unit in the solution.<\/li>\n            <li>(B) i = 5, because it dissociates into four potassium ions and one ferrocyanide complex ion.<\/li>\n            <li>(C) i = 10, because every single atom in the formula becomes an independent particle in the water.<\/li>\n            <li>(D) i = 4, because only the potassium ions contribute to the colligative properties of the solution.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 19 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q19.<\/strong> Which of the following best describes the effect of increasing external pressure on the solubility of a solid in a liquid?<\/p>\n        <ul>\n            <li>(A) Solubility increases significantly because the pressure forces the solid particles into the spaces between liquid molecules.<\/li>\n            <li>(B) Solubility decreases because high pressure stabilizes the solid crystal lattice, making it harder to break.<\/li>\n            <li>(C) There is practically no effect because solids and liquids are highly incompressible and their volumes do not change much.<\/li>\n            <li>(D) The solid will immediately precipitate because pressure always favors the state with the highest density.<\/li>\n        <\/ul>\n    <\/div>\n\n    <!-- Question 20 -->\n    <div class=\"question-block\" style=\"margin-bottom: 30px;\">\n        <p><strong>Q20.<\/strong> If the Molal Elevation Constant (K<sub>b<\/sub>) for water is 0.52 K kg\/mol, what does this value physically represent?<\/p>\n        <ul>\n            <li>(A) The temperature at which one kilogram of pure water will begin to boil at standard atmospheric pressure.<\/li>\n            <li>(B) The increase in boiling point when one mole of a non-volatile, non-electrolyte solute is dissolved in one kilogram of water.<\/li>\n            <li>(C) The amount of heat energy required to vaporize one mole of water from a 1 molal solution.<\/li>\n            <li>(D) The maximum concentration of solute that can be added to water before the boiling point stops rising.<\/li>\n        <\/ul>\n    <\/div>\n<\/div>\n\n\n\n<div class=\"gk-resource-footer\" style=\"padding: 20px; border-radius: 12px; background-color: #f8f9fa; border: 1px solid #e1e4e8; font-family: 'Segoe UI', Roboto, Helvetica, Arial, sans-serif; text-align: center; margin-top: 30px;\">\n    \n    <h3 style=\"color: #2c3e50; margin-bottom: 20px; font-weight: 700; text-transform: uppercase; letter-spacing: 1px;\">Class XII Chemistry Resources<\/h3>\n    \n    <div style=\"display: flex; flex-wrap: wrap; justify-content: center; gap: 15px; margin-bottom: 25px;\">\n        <!-- Easy Level -->\n        <a target=\"_blank\" href=\"https:\/\/gyankatta.co.in\/ma\/mod\/quiz\/view.php?id=420\" style=\"text-decoration: none; padding: 12px 20px; background: #28a745; color: white; border-radius: 8px; font-weight: 600; min-width: 180px; box-shadow: 0 4px 6px rgba(40, 167, 69, 0.2); transition: transform 0.2s;\">\n            Solutions (Easy)\n        <\/a>\n\n        <!-- Moderate Level -->\n        <a target=\"_blank\" 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A student observes that a mixture of Chloroform and Acetone becomes noticeably warm during the mixing process. Which of the following best explains the molecular behavior and the resulting vapor pressure of this solution? (A) The mixture shows a positive deviation from Raoult\u2019s Law [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":163038,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"fifu_image_url":"https:\/\/manishchandra.org\/p7\/cl12ChemSolutionsporster.png","fifu_image_alt":"","footnotes":""},"categories":[28,58,3],"tags":[],"class_list":["post-163035","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-chemistry","category-class-xii-chemistry","category-education","cat-28-id","cat-58-id","cat-3-id","has_thumb"],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v27.5 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>Class 12 Chemistry: Solutions - Advanced Challenge (ASSET Pro Max) - Gyankatta<\/title>\n<meta name=\"description\" content=\"Gyankatta Class 12 Chemistry: Solutions - Advanced Challenge (ASSET Pro Max) education https:\/\/news.gyankatta.org\/?p=163035\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/news.gyankatta.org\/?p=163035\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Class 12 Chemistry: Solutions - Advanced Challenge (ASSET Pro Max) - Gyankatta\" \/>\n<meta property=\"og:description\" content=\"Gyankatta Class 12 Chemistry: Solutions - Advanced Challenge (ASSET Pro Max) education https:\/\/news.gyankatta.org\/?p=163035\" \/>\n<meta property=\"og:url\" content=\"https:\/\/news.gyankatta.org\/?p=163035\" \/>\n<meta property=\"og:site_name\" content=\"Gyankatta\" \/>\n<meta property=\"article:published_time\" content=\"2026-05-03T04:36:56+00:00\" \/>\n<meta property=\"article:modified_time\" content=\"2026-05-03T05:27:56+00:00\" \/>\n<meta property=\"og:image\" content=\"https:\/\/manishchandra.org\/p7\/cl12ChemSolutionsporster.png\" \/>\n<meta name=\"author\" content=\"sBagul\" \/>\n<meta name=\"twitter:card\" content=\"summary_large_image\" \/>\n<meta name=\"twitter:image\" content=\"https:\/\/manishchandra.org\/p7\/cl12ChemSolutionsporster.png\" \/>\n<meta name=\"twitter:label1\" content=\"Written by\" \/>\n\t<meta name=\"twitter:data1\" content=\"sBagul\" \/>\n\t<meta name=\"twitter:label2\" content=\"Est. reading time\" \/>\n\t<meta name=\"twitter:data2\" content=\"10 minutes\" \/>\n<script type=\"application\/ld+json\" class=\"yoast-schema-graph\">{\"@context\":\"https:\\\/\\\/schema.org\",\"@graph\":[{\"@type\":\"Article\",\"@id\":\"https:\\\/\\\/news.gyankatta.org\\\/?p=163035#article\",\"isPartOf\":{\"@id\":\"https:\\\/\\\/news.gyankatta.org\\\/?p=163035\"},\"author\":{\"name\":\"sBagul\",\"@id\":\"https:\\\/\\\/news.gyankatta.org\\\/#\\\/schema\\\/person\\\/ba6f7a4ee74e137c4c2b2c991b4f28e9\"},\"headline\":\"Class 12 Chemistry: Solutions &#8211; 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