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Solutions, Suspensions, and Colloids Solved MCQs in Chemistry

 Solutions, Suspensions, & Colloids

Solutions, Suspensions and Colloids

1. Which of the following is a heterogeneous mixture?

   a) Saltwater

   b) Air

   c) Sand in water

   d) Sugar in water  


2. What does the term "solute" refer to in a solution?

   a) The substance that is dissolved

   b) The substance that does the dissolving

   c) The resulting mixture

   d) The solvent  


3. Which factor does NOT affect the solubility of a solid solute in a solvent?

   a) Temperature

   b) Pressure

   c) Surface area

   d) Nature of solute and solvent  

  

4. What happens to the boiling point of a solution compared to the pure solvent?

   a) It decreases

   b) It increases

   c) It remains the same

   d) It varies depending on the solute  


5. Which term is used to describe a solution that has reached its maximum amount of solute at a given temperature?

   a) Dilute solution

   b) Concentrated solution

   c) Saturated solution

   d) Supersaturated solution  


6. What is the solvent in an aqueous solution?

   a. Water  

   b. Salt  

   c. Sugar  

   d. Alcohol  


7. Which of the following is a solute in a solution of saltwater?

   a. Water  

   b. Sodium chloride  

   c. Oxygen  

   d. Hydrogen  


8. A solution with a large amount of solute compared to the solvent is called:

   a. Dilute solution  

   b. Concentrated solution  

   c. Saturated solution  

   d. Unsaturated solution  


9. What does the term "aqueous" in an aqueous solution indicate?

   a. It contains air  

   b. It is acidic  

   c. It is a solid  

   d. It contains water  


10. In a solution, the substance present in the smallest amount is called the:

   a. Solvent  

   b. Solute  

   c. Mixture  

   d. Compound  


11. What is the maximum amount of solute that can dissolve in a solvent at a given temperature, forming a saturated solution?

   a. Solubility  

   b. Concentration  

   c. Saturation point  

   d. Density  


 12. Which of the following is an example of a non-aqueous solution?

   a. Saltwater  

   b. Sugar dissolved in water  

   c. Alcohol in water  

   d. Oil in water  


13. What happens to the solubility of most solid solutes as the temperature of the solvent increases?

   a. It increases  

   b. It decreases  

   c. It remains constant  

   d. It depends on the specific solute  


14. A solution that has more solute dissolved than it would normally hold at a specific temperature is termed:

   a. Dilute solution  

   b. Concentrated solution  

   c. Supersaturated solution  

   d. Unsaturated solution  


15. Which term refers to a mixture that has uniform composition and properties throughout?

    a. Compound  

    b. Element  

    c. Solution  

    d. Suspension  


16. What term describes a solution that contains the maximum amount of solute that can dissolve at a given temperature?

   a. Unsaturated solution  

   b. Saturated solution  

   c. Supersaturated solution  

   d. Diluted solution  


17. Which of the following statements is true about an unsaturated solution?

a. It contains more solute than can dissolve.  

b. It contains less solute than can dissolve.  

c. It is in equilibrium with undissolved solute.  

   d. It is always a clear solution.


18. What type of solution can dissolve additional solute at a given temperature?

   a. Saturated solution  

   b. Unsaturated solution  

   c. Supersaturated solution  

   d. Diluted solution  


19. In a supersaturated solution, what is the typical result if a small crystal of solute is added?

   a. No change occurs.  

 b. Precipitation of excess solute occurs.  

  c. The solution becomes more unsaturated.  

   d. The solution becomes cloudy.


20. What process involves adding more solvent to a solution, resulting in a decrease in the concentration of the solute?

   a. Saturation  

   b. Dilution  

   c. Supersaturation  

   d. Precipitation  


21. What type of solution is formed when a gas dissolves in a liquid?

   a) Solid solution

   b) Liquid solution

   c) Gaseous solution

   d) Aqueous solution


22. Which of the following is an example of a solid-liquid solution?

    a) Saltwater

    b) Air

    c) Brass (copper-zinc alloy)

    d) Carbonated water


23. What is the solvent in a solution of sugar dissolved in water?

    a) Sugar

    b) Water

    c) Mixture

   d) None of the above


24. A solution with a high concentration of solute is termed as:

   a) Dilute

   b) Concentrated

   c) Saturated

   d) Unsaturated


25. What type of solution is formed when no more solute can dissolve in a solvent at a given temperature?

    a) Unsaturated solution

    b) Saturated solution

    c) Dilute solution

   d) Concentrated solution


6. When sugar is dissolved in water, the resulting solution is classified as:

    a) Homogeneous

   b) Heterogeneous

   c) Colloidal

   d) Suspension


 27. Which of the following is an example of a gas-gas solution?

   a) Air

   b) Vinegar

   c) Soda water

   d) Brass


28. What is the process by which a solute comes out of solution and forms crystals?

   a) Dissolution

   b) Precipitation

   c) Evaporation

   d) Filtration


29. A solution with equal amounts of solute and solvent is called:

    a) Saturated

    b) Dilute

    c) Unsaturated

    d) Concentrated


30. Which of the following does NOT affect the rate of solubility of a solute in a solvent?

    a) Temperature

    b) Pressure

    c) Particle size of solute

    d) Color of solute


31. What is the definition of an aqueous solution in chemistry?

a. A solution that contains water as the solvent

b. A solution that contains a gas as the solute

 c. A solution that is highly acidic

 d. A solution that only contains solid solutes


32. Which of the following is an example of a solute in a solution?

   a. Water

   b. Salt

   c. Sugar

   d. Both a and b


33. In the solution, HCl(aq), what does "(aq)" represent?

   a. Aqueous

   b. Acid

   c. Acquired

   d. Alcohol


34. What is the solvent in a solution where ethanol is dissolved in water?

   a. Ethanol

   b. Water

   c. Both equally

   d. Neither


35. Which concentration unit is defined as moles of solute per liter of solution?

   a. Molarity (M)

   b. Molality (m)

   c. Mass percent (% mass)

   d. Volume percent (% volume)


36. What is the formula for calculating mass percent (% mass) of a solute in a solution?

a. (Mass of solute / Mass of solution) x 100

b. (Volume of solute / Volume of solution) x 100

c. (Moles of solute / Moles of solution) x 100

d. (Density of solute / Density of solution) x 100


37. Which concentration unit is temperature-dependent and is often used when dealing with colligative properties?

   a. Molarity (M)

   b. Molality (m)

   c. Mass percent (% mass)

   d. Volume percent (% volume)


 38. What does ppm stand for in the context of concentration units?

   a. Parts per million

   b. Percentage per molecule

   c. Purity per mass

   d. Particle per mixture


39. Which concentration unit is calculated as the ratio of the volume of solute to the total volume of the solution multiplied by 100?

   a. Molarity (M)

   b. Molality (m)

   c. Mass percent (% mass)

   d. Volume percent (% volume)


40. If you dissolve 10 grams of salt in 100 grams of water, what is the mass percent of salt in the solution?

   a. 10%

   b. 20%

   c. 30%

   d. 40%


41. What is the definition of solubility in chemistry?

a. The ability of a substance to dissolve in a solvent  

b. The measure of a substance's weight  

c. The temperature at which a substance changes state  

d. The ability of a solvent to evaporate


42. Which of the following is known as the universal  solvent?

a. Sodium Chloride 

b. Sulphuric Acid  

c. Hydrochloric Acid 

d. Water 


43. Which of the following statements is true regarding the solubility of gases in liquids?

a. Solubility of gases decreases with increasing temperature  

b. Solubility of gases is unaffected by pressure  

c. Solubility of gases generally increases with increasing pressure

d. Solubility of gases is independent of the nature of the gas


44. What is the term for a solution that contains the maximum amount of solute that can dissolve at a given temperature?

a. Unsaturated solution  

b. Saturated solution 

c. Dilute solution  

d. Supersaturated solution  


45. The solubility of most solid solutes in water tends to increase with:

a. Decreasing temperature  

b. Constant pressure  

c. Increasing temperature  

d. Unchanged particle size


46. In a solution, the component present in lesser quantity is called:

a. Solvent  

b. Solute  

c. Solution  

d. Trace element


47. Henry's law is related to the solubility of:

a. Liquids in liquids  

b. Gases in liquids  

c. Solids in liquids  

d. Gases in solids


48. The solubility of most gases in water follows which pattern as temperature increases?

a. Decreases  

b. Increases  

c. Remains constant  

d. Depends on the nature of the gas


49. Which of the following is a qualitative measure of the concentration of a solution?

a. Molality  

b. Molarity  

c. Dilution  

d. Saturation


50. What happens to the solubility of most solid solutes as pressure increases?

a. Increases  

b. Decreases  

c. Remains constant  

d. Depends on the nature of the solute


51. What is the term used to describe a homogeneous mixture of two or more substances, typically with water as the solvent?

   a) Compound  

   b) Element  

   c) Solution  

   d) Suspension  


52. Which of the following is an example of a non-polar solvent?

   a) Water  

   b) Ethanol  

   c) Hexane  

   d) Acetone  


53. The process by which a solute dissolves in a solvent to form a solution is called:

   a) Precipitation  

   b) Sublimation  

   c) Dissociation  

   d) Dissolution  


54. What factors affect the solubility of a solute in a solvent?

   a) Temperature and pressure  

   b) Density and viscosity  

   c) Color and odor  

   d) pH and conductivity 


55. Which statement is true about the solubility of most solid solutes in water?

a) Solubility decreases with increasing temperature  

b) Solubility increases with increasing temperature  

 c) Temperature has no effect on solubility  

 d) Solubility is only affected by pressure  


56. The interaction between solute and solvent molecules that involves the formation of hydrogen bonds is most likely to occur when the solute is:

   a) Ionic  

   b) Non-polar  

   c) Covalent  

   d) Metallic  


57. Which of the following is an example of a saturated solution?

a) A solution with undissolved solute at the bottom  

b) A solution with dissolved solute at the bottom  

c) A solution with the maximum amount of solute dissolved  

d) A solution with equal amounts of solute and solvent  


58. What is the term for the maximum amount of solute that can dissolve in a solvent at a specific temperature?

   a) Concentration  

   b) Saturation  

   c) Dilution  

   d) Viscosity  


59. Which type of solution has more solute dissolved than a saturated solution at a given temperature?

   a) Unsaturated  

   b) Saturated  

   c) Supersaturated  

   d) Dilute  


60. Henry's law describes the relationship between the pressure of a gas and its solubility in a liquid. What happens to the solubility of a gas in a liquid when the pressure is increased?

   a) Solubility increases  

   b) Solubility decreases  

   c) Solubility remains unchanged  

   d) Solubility depends on the type of gas  


61. What is a defining characteristic of a solution in chemistry?

   a) Heterogeneous mixture  

   b) Particles settle over time  

   c) Homogeneous mixture  

   d) Large particle size  


62. In an aqueous solution, what does the term "solute" refer to?

   a) The substance dissolved in water  

   b) The substance doing the dissolving  

   c) The water itself  

   d) Any gas present in the solution  


63. What distinguishes a suspension from a solution?

   a) Small particle size  

   b) Homogeneous composition  

   c) Particles do not settle  

   d) Heterogeneous composition  


64. What is a characteristic feature of colloids in comparison to solutions and suspensions?

   a) Small particle size  

   b) Clear separation of components  

   c) Particles settle quickly  

   d) Homogeneous composition  


65. Which of the following statements is true about solutions?

   a) They scatter light  

   b) They are always opaque  

   c) They settle upon standing  

   d) They have a uniform composition  


66. What is the primary factor influencing the stability of colloids?

   a) Particle size  

   b) Temperature  

   c) Pressure  

   d) Density  


67. Which type of mixture is characterized by particles that settle over time?

   a) Solution  

   b) Suspension  

   c) Colloid  

   d) Emulsion  


68. In a solution, what does the term "solubility" refer to?

   a) The ability of the solvent to dissolve  

b) The amount of solute that can dissolve in a given solvent at a specific temperature  

   c) The concentration of the solute  

   d) The volume of the solution  


69. Which type of mixture has particles that can be separated through filtration?

   a) Solution  

   b) Suspension  

   c) Colloid  

   d) Emulsion  


70. What is a colloid in chemistry?

a) Homogeneous mixture  

b) Heterogeneous mixture  

c) Pure substance  

d) Element


71. Which of the following is an example of a colloidal system?

a) Saltwater  

b) Lemonade  

c) Milk  

d) Distilled water


72. What is the size range of particles in a colloid?

a) Greater than 1 mm  

b) Between 1 nm and 100 nm  

c) Less than 1 nm  

d) Exactly 1 μm


73. The process of settling down of colloidal particles is known as:

a) Precipitation  

b) Sedimentation  

c) Filtration  

d) Coagulation


74. What is the Tyndall effect in colloids?

a) Dispersion of light by colloidal particles  

b) Precipitation of colloids  

c) Sedimentation of colloids  

d) Coagulation of colloids


75. Which of the following is a common method to stabilize a colloidal solution?

a) Filtration  

b) Sedimentation  

c) Electrophoresis  

d) Addition of electrolytes


76. The process of converting a sol into a gel is known as:

a) Precipitation  

b) Coagulation  

c) Peptization  

d) Sedimentation


77. What is the primary factor influencing the viscosity of colloidal solutions?

a) Temperature  

b) Particle size  

c) Pressure  

d) Concentration


78. Which of the following is an example of a lyophilic sol?

a) Starch in water  

b) Silver iodide in water  

c) Gum in water  

d) Sand in water


79. What happens to the charge on colloidal particles during coagulation?

a) No change  

b) Increases  

c) Decreases  

d) Becomes neutral


80. How do colloids differ from solutions and suspensions?

a) Colloids have larger particles than suspensions  

b) Colloids scatter light, while solutions do not  

c) Solutions have visible particles, unlike colloids  

d) Suspensions do not exhibit the Tyndall effect  


81. What is a common scientific application of colloids?

a) Making lemonade  

b) Blood transfusion  

c) Filtration of tap water  

d) Dissolving sugar in tea  


82. Which type of mixture is most commonly used in technological applications like ink and paint?

a) Solution  

b) Suspension  

c) Colloid  

d) Compound  


83. What property distinguishes a solution from a colloid?

a) Particle size  

b) Transparency  

c) Settling rate  

d) Solubility  


84. Why do solutions conduct electricity?

a) Due to the presence of solutes  

b) Because of the solvent's conductivity  

c) Solutions do not conduct electricity  

d) Only ionic solutions conduct electricity  


85. What is the primary factor influencing the rate at which a solute dissolves in a solvent?

a) Temperature  

b) Pressure  

c) Color  

d) Density  


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Solutions, Collids, and Suspension Notes

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Acids, Bases, and Salts Notes

Chemistry and Branches of Chemistry Solved MCQs 

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