Preparing for the Joint Entrance Exam (JEE) can be a daunting task. With so many subjects to cover and so many topics to study, it can be challenging to know where to start. One essential topic in the JEE Mains syllabus is the Solutions. In this article, we will provide 50+ MCQ questions on the Solutions, along with detailed solutions to help you prepare for the JEE Mains exam.
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These 50+ MCQ questions are selected by the experts of studyrate.in and these are more difficult questions, which will help you to better understand Solutions JEE Mains MCQ Questions with Answers.
Solutions JEE Mains MCQ
Which of the following compounds shows the highest degree of solubility in water? a) Sodium chloride (NaCl) b) Sodium bromide (NaBr) c) Sodium iodide (NaI) d) Sodium fluoride (NaF)
Answer: a) Sodium chloride (NaCl)
Explanation: The degree of solubility in water depends on the strength of the ionic bond. Among the given compounds, sodium chloride (NaCl) has the highest degree of solubility in water due to its strong ionic bond.
The solubility of gases in liquids generally: a) Increases with an increase in temperature b) Decreases with an increase in temperature c) Remains constant with temperature d) Depends on the nature of the gas
Answer: b) Decreases with an increase in temperature
Explanation: The solubility of gases in liquids generally decreases with an increase in temperature. This is because as the temperature rises, the kinetic energy of gas molecules increases, leading to a decrease in their solubility in the liquid.
Which of the following factors does not affect the rate of dissolution of a solute in a solvent? a) Temperature b) Surface area of the solute c) Pressure d) Density of the solvent
Answer: d) Density of the solvent
Explanation: The density of the solvent does not directly affect the rate of dissolution of a solute in a solvent. Factors such as temperature, surface area of the solute, and pressure can influence the rate of dissolution.
Which of the following solutions will show the highest boiling point elevation? a) 0.1 M NaCl b) 0.1 M glucose (C6H12O6) c) 0.1 M MgCl2 d) 0.1 M CaCl2
Answer: d) 0.1 M CaCl2
Explanation: The boiling point elevation depends on the number of particles (ions or molecules) in the solution. CaCl2 dissociates into three particles (1 Ca2+ and 2 Cl-) in water, resulting in the highest boiling point elevation compared to the other options.
The concentration of a solution is usually expressed in: a) Mass/volume b) Moles/volume c) Moles/mass d) Volume/moles
Answer: b) Moles/volume
Explanation: The concentration of a solution is commonly expressed in moles of solute per unit volume of the solution, such as moles per liter (Molarity, M).
The colligative property of a solution that depends on the total number of solute particles is: a) Vapor pressure lowering b) Boiling point elevation c) Freezing point depression d) Osmotic pressure
Answer: c) Freezing point depression
Explanation: Freezing point depression is a colligative property that depends on the total number of solute particles in the solution. It is observed as a lower freezing point compared to the pure solvent.
The Raoult’s law is applicable to: a) Ideal solutions b) Non-ideal solutions c) Only binary solutions d) Solutions at high temperatures
Answer: a) Ideal solutions
Explanation: Raoult’s law is applicable to ideal solutions, which are characterized by obeying the laws of ideal behavior. It describes the vapor pressure of each component in an ideal solution as proportional to its mole fraction in the solution.
Which of the following statements about azeotropes is incorrect? a) Azeotropes have constant boiling compositions. b) Azeotropes can be separated by simple distillation. c) Azeotropes exhibit maximum or minimum boiling points. d) Azeotropes have vapor compositions different from their liquid compositions.
Answer: b) Azeotropes can be separated by simple distillation.
Explanation: Azeotropes cannot be separated by simple distillation because they have constant boiling compositions. Simple distillation is only effective for separating components with different boiling points.
The presence of a non-volatile solute in a solvent results in: a) Decreased boiling point of the solvent b) Increased boiling point of the solvent c) No effect on the boiling point of the solvent d) Increased vapor pressure of the solvent
Answer: b) Increased boiling point of the solvent
Explanation: The presence of a non-volatile solute in a solvent increases the boiling point of the solvent. This phenomenon is known as boiling point elevation, which is a colligative property.
Which of the following is an example of a non-electrolyte? a) Sodium chloride (NaCl) b) Hydrochloric acid (HCl) c) Glucose (C6H12O6) d) Sodium hydroxide (NaOH)
Answer: c) Glucose (C6H12O6)
Explanation: Glucose (C6H12O6) is an example of a non-electrolyte because it does not dissociate into ions when dissolved in water. It remains as intact molecules in solution.
The process of removing dissolved salts from seawater to obtain fresh water is known as: a) Distillation b) Filtration c) Evaporation d) Reverse osmosis
Answer: d) Reverse osmosis
Explanation: Reverse osmosis is the process of removing dissolved salts and impurities from seawater or brackish water to obtain fresh water. It involves the use of a semipermeable membrane to selectively allow water molecules to pass while blocking the passage of salts.
The solubility of a gas in a liquid generally: a) Increases with an increase in pressure b) Decreases with an increase in pressure c) Remains constant with pressure d) Depends on the nature of the gas
Answer: a) Increases with an increase in pressure
Explanation: The solubility of a gas in a liquid generally increases with an increase in pressure. This is described by Henry’s law, which states that the solubility of a gas is directly proportional to the partial pressure of the gas above the liquid.
Which of the following mixtures is an example of a heterogeneous mixture? a) Saltwater b) Air c) Brass (an alloy of copper and zinc) d) Milk
Answer: d) Milk
Explanation: Milk is an example of a heterogeneous mixture because it consists of visibly distinct phases, such as fat globules dispersed in a liquid matrix.
Which of the following is an example of a supersaturated solution? a) A saturated solution at room temperature b) A solution with a concentration of 0.5 M c) A solution with a concentration below the solubility limit d) A solution with excess solute dissolved beyond its solubility limit
Answer: d) A solution with excess solute dissolved beyond its solubility limit
Explanation: A supersaturated solution is a solution that contains more dissolved solute than what is normally possible at a given temperature. It is achieved by dissolving excess solute at an elevated temperature and then cooling the solution without allowing the excess solute to precipitate.
The molarity of a solution is defined as: a) The mass of solute dissolved in a given volume of solvent b) The volume of solute dissolved in a given mass of solvent c) The number of moles of solute dissolved in a given volume of solution d) The number of moles of solute dissolved in a given mass of solvent
Answer: c) The number of moles of solute dissolved in a given volume of solution
Explanation: Molarity (M) is defined as the number of moles of solute dissolved in one liter (or cubic decimeter) of solution.
Which of the following is an example of a colligative property? a) Color of a solution b) pH of a solution c) Density of a solution d) Boiling point of a solution
Answer: d) Boiling point of a solution
Explanation: Colligative properties are properties of a solution that depend on the number of solute particles present, regardless of their chemical nature. The boiling point of a solution is an example of a colligative property.
The process of the spontaneous net movement of solvent molecules through a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration is called: a) Osmosis b) Diffusion c) Filtration d) Dialysis
Answer: a) Osmosis
Explanation: Osmosis is the process of the spontaneous net movement of solvent molecules (usually water) through a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration.
The Tyndall effect is observed in: a) True solutions b) Colloidal solutions c) Suspension d) All of the above
Answer: b) Colloidal solutions
Explanation: The Tyndall effect is the scattering of light by the dispersed phase of a colloidal solution. It is observed in colloidal solutions but not in true solutions or suspensions.
The process of converting a solution into a solid by removing the solvent is called: a) Crystallization b) Decantation c) Filtration d) Sublimation
Answer: a) Crystallization
Explanation: Crystallization is the process of converting a solution into a solid by removing the solvent. It involves cooling the solution or evaporating the solvent to induce the formation of crystals.
The process of separating the components of a mixture based on their different solubilities in a particular solvent is called: a) Filtration b) Chromatography c) Distillation d) Decantation
Answer: b) Chromatography
Explanation: Chromatography is a process used for separating the components of a mixture based on their different solubilities and affinities for a particular solvent or mobile phase. It is widely used in chemical analysis and purification techniques.
Which of the following statements about ideal solutions is correct? a) The enthalpy of mixing is zero for ideal solutions. b) The vapor pressure of each component is independent of its mole fraction. c) The volume of the solution is always equal to the sum of the volumes of the individual components. d) The boiling point of the solution is always higher than the boiling points of the individual components.
Answer: b) The vapor pressure of each component is independent of its mole fraction.
Explanation: In an ideal solution, the vapor pressure of each component is independent of its mole fraction. This is one of the defining characteristics of an ideal solution.
Which of the following factors does not affect the rate of dissolution of a solute in a solvent? a) Temperature b) Surface area of the solute c) Pressure d) Density of the solvent
Answer: d) Density of the solvent
Explanation: The density of the solvent does not directly affect the rate of dissolution of a solute in a solvent. Factors such as temperature, surface area of the solute, and pressure can influence the rate of dissolution.
The presence of a non-volatile solute in a solvent results in: a) Decreased boiling point of the solvent b) Increased boiling point of the solvent c) No effect on the boiling point of the solvent d) Increased vapor pressure of the solvent
Answer: b) Increased boiling point of the solvent
Explanation: The presence of a non-volatile solute in a solvent increases the boiling point of the solvent. This phenomenon is known as boiling point elevation, which is a colligative property.
The boiling point elevation of a solution is directly proportional to: a) The molar mass of the solute b) The volume of the solute c) The concentration of the solute d) The density of the solute
Answer: c) The concentration of the solute
Explanation: The boiling point elevation of a solution is directly proportional to the concentration of the solute. A higher concentration of solute leads to a greater increase in boiling point.
Which of the following is an example of an electrolyte? a) Ethanol (C2H5OH) b) Glucose (C6H12O6) c) Sodium chloride (NaCl) d) Benzene (C6H6)
Answer: c) Sodium chloride (NaCl)
Explanation: Sodium chloride (NaCl) is an example of an electrolyte because it dissociates into ions (Na+ and Cl-) when dissolved in water, allowing for the conduction of electricity.
The phenomenon of adsorption is characterized by: a) The formation of a homogeneous mixture between solute and solvent. b) The formation of a monolayer of solute molecules on the surface of the solvent. c) The formation of a precipitate due to the insolubility of the solute. d) The separation of solute particles from a mixture by centrifugation.
Answer: b) The formation of a monolayer of solute molecules on the surface of the solvent.
Explanation: Adsorption refers to the accumulation of a solute on the surface of a solvent or solid. It involves the formation of a monolayer of solute molecules on the surface of the solvent.
Which of the following is an example of a suspension? a) Orange juice b) Vinegar c) Air d) Muddy water
Answer: d) Muddy water
Explanation: Muddy water is an example of a suspension because it contains visible particles (mud or soil) that are dispersed in the liquid phase.
The process of converting a gas directly into a solid without going through the liquid state is called: a) Condensation b) Evaporation c) Sublimation d) Precipitation
Answer: c) Sublimation
Explanation: Sublimation is the process of converting a substance from the solid state directly into the gas state without passing through the liquid state. It is a phase transition that occurs under specific temperature and pressure conditions.
The Henry’s law constant is a measure of: a) Solubility b) Boiling point elevation c) Freezing point depression d) Osmotic pressure
Answer: a) Solubility
Explanation: The Henry’s law constant (kH) is a measure of the solubility of a gas in a liquid. It relates the concentration of a gas in a solution to its partial pressure in the gas phase.
The process of separating the components of a liquid mixture based on their different boiling points is called: a) Filtration b) Distillation c) Crystallization d) Chromatography
Answer: b) Distillation
Explanation: Distillation is the process of separating the components of a liquid mixture based on their different boiling points. It involves heating the mixture to vaporize the more volatile component and then condensing the vapor to obtain the purified component.
We hope there JEE MCQ of Class 12 : Solutions will help you to score an excellent rank in JEE Mains and Advanced. If you have any queries feel free to write in the comments section. We at Study Rate are always ready to serve our students.
