{"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&#8230;<\/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"],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v27.6 - 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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