1st Year Chemistry Solutions MCQs with Answers

This is the place where you will get 1st Year Chemistry Solutions MCQs with Answers. A solution is made by mixing two or more different types of substances. Solutions have different types of concentration Units. These units include Molality, Mole fractions, and Molarity. Solutions have types that differ from the mixing of types of Matter. Raoult’s law has much interference in Solutions. The percentage or amount of solute added in solution is termed as Solubility. Solutions have their different Colligative Properties. Hydration and Hydrolysis tell us about the interactions of different ions, salts, and other particles of Solution. So, this is the brief introduction of this chapter. Scroll down to get the important MCQs of this chapter.

1st Year Chemistry Solutions MCQs with Answers

KEY POINTS

 

Question#1. 10g NaOH is dissolved in 1000g water. The molality of NaOH is:

• 1m
• 0.5m
• 4m
• 0.25m

Question#2. 250cm³ of 0.2 molar potassium sulphate solution is mixed with 250cm³ of 0.2 molar KCl solution. The molar concentration of K⁺ ions is:

• 0.2 molar
• 0.3 molar
• 0.25 molar
• 0.35 molar

Question#3. The molality of pure water is:

• 1
• 55.5
• 18
• 6

Question#4. Molal boiling point constant is the ratio of the elevation in the boiling to:

• Molarity
• Mole fraction of solvent
• Molality
  
• Mole fraction of the solute

Question#5. The number of molecules of sugar in 1dm³ of 1M sugar solution is:

• 6.02 x 10²³
• 3.42 x 6.02 x 10²²
• 6.02 x 10²⁰
• None of the above

Question#6. Colligative properties can be used for calculating:

• The density of a compound
• The lattice energy of a compound
• The molecular mass of a compound
• All of the above

Question#7. 18g glucose is dissolved in 90g water. The relative lowering of vapor pressure is equal to:

• 1/5
• 1/51
• 5.1
• 1/55.5

Question#8. A solution has 92g ethanol, 96g methanol, and 90g water. Mole fraction of water in the solution is:

• 0.1
• 0.4
• 0.2
• 0.5

Question#9. Elevation of boiling point can be best studied by:

• Beckmann’s method
•  Landsberger’s method
• Gibb’s method
• None of the above

Question#10. For observing Colligative properties, which of the following conditions should be fulfilled?

• The solution should be dilute
• Solute should be non-electrolyte
• Solute should be non-volatile
• All of the above

Question#11. When the solvent is containing non-volatile solute particles, then:

• Vapor pressure is decreased
• Vapor pressure doesn’t change
• Vapor pressure is elevated
• Volume is decrease

Question#12. The freezing point is the temperature of the substance at which its solid and liquid phases have the:

• Different vapor pressure
• Same volume
• Same vapor pressure
• Same density

Qv13. A solution of glucose is 10%. The volume in which 1g mole of it will be dissolved is:

• 1 dm³
• 200 dm³
• 1.8 dm³
• 180 dm³

Question#14. Which of the following is not a colligative property?

• Density
  
• Elevation of boiling point
• Depression in freezing point
• Osmotic pressure

Question#15. The substances which don’t dissolve in a reasonable amount in a particular solvent are_____.

• Miscible
• Well soluble
• Sparingly soluble
• Insoluble

Question#16. Which one of the following solution of glucose in water is more dilute?

• 0.1 molar
• 0.1 molal
• 1% w/w
• All have the same concentration

Qv17. Which liquid solute is dissolved in the liquid solvent, then the best unit of concentration is?

• % w/w
• % w/v
• % v/v
• % v/w

Question#18. Which of the following is an example of solid in solid solution?

• Dust particles in smoke
• Opals
  
• Mercury metal in silver metal
• All of the above

Question#19. A colligative property is not represented by:

• Elevation of boiling point
• Osmotic pressure
• Freezing point
• Relative lowering of vapor pressure

Question#20. A solution of KCl in water contains:

• Free formula units
• Free ions
• Free atoms
• Free molecules

Question#21. For very dilute solution the following expression is used:

• Gram per million
• Nanogram per million
• Microgram per million
• Parts per million

Question#22. That solution which possesses a maximum concentration of solute at a given temperature is known as:

• Unsaturated
• Saturated
  
• Supersaturated
• Dilute solution

Question#23. Which of the following 0.1 m solution will have the lowest freezing point?

• K₂SO₄
• NaCl
• Glucose
• Urea

Question#24. Which has the highest freezing point?

• 1.0 m NaCl
• 1.0 m CaCl₂
• 1.0 m Urea
• 1.0 m KCl

Question#25. Which of the following statement is true about ideal solutions?

• The change in volume is zero
• The change in enthalpy is zero
• The vapor pressure change is zero
• Both a and b

Question#26. The addition of sodium chloride to water, while boiling eggs results to:

• Decrease boiling point of water
• Increase the boiling point of water
• Prevent breaking of eggs
• Make egg tasty

Question#27. Which pair of the following will not form an ideal solution?

• C₂H₅Br + C₂H₅I
• H₂O + C₄H₉OH
• C₆H₁₄ + C₇H₁₆
• CCl₄ + SiCl₄

Question#28. The study of elevation of boiling point is called:

• Ebullioscopy
• Cryoscopy
• Osmometer
• None of these

Question#29. A solution of glucose is 10% w/v. The volume in which 1g mole of it is dissolved will be:

• 1dm³
• 200 cm³
• 900 cm³
• 1.8 dm³

Question#30. The relative lowering of vapor pressure is equal to:

• Mole fraction of solvent
• Mole fraction of solution
• The molar mass of solute
• Mole fraction of solute