We rarely come across pure substances in everyday life.The majority of these are mixtures of two or more pure substances. Their utility or significance in life is determined by their composition. For example, the properties of brass (a mixture of copper and zinc) differ significantly from those of German silver (a mixture of copper, zinc, and nickel) or bronze (a mixture of copper and tin).
Download Class 12 Chemistry Worksheet on Chapter 2 Solutions Set 1 PDF
CBSE Class 12 Chemistry Chapter 2 Solutions Worksheet – Set 1
Q-1: A mixture contains 1 mole of volatile liquid A(PoA=100 mm Hg) and 3 moles of volatile liquid B(PBo=80 mm Hg). If solution behave ideally, the total vapour pressure of the distillate is
a) 85 mm Hg
b) 85.88 mm Hg
c) 90 mm Hg
d) 92 mm Hg
Q-2: Which of the following represents correctly the changes in thermodynamic properties during the formation of 1 mole of an ideal binary solution?
Q-3: The vapour pressure of pure liquid A is 10 Torr and at the same temperature when 1 g of B solid is dissolved in 20 g of A, its vapour pressure is reduced to 9.0 torr. If the molecular mass of A is 200 amu, then the molecular mass of B is:
a) 100 amu
b) 90 amu
c) 75 amu
d) 120 amu
Q-4: The correct relationship between the boiling points of very dilute solutions of AlCl3(T1K) and CaCl2 (T2K) having the same molar concentration is
a) T1=T2
b) T1 >T2
c) T2 >T1
d) T2 ≤T1
Q-5:Define the term azeotrope.Give one example of a minimum boiling azeotrope.
Q-6: Why is the liquid ammonia bottle cooled in ice before being opened?
Q-7: In thermogravimetric analysis, a sample of 25 mg hydrated compound (molecular weight = 250g/mol) yields 16 mg of dehydrated compound. The number of water molecules lost per hydrated compound molecule is_________. (Water has a molecular weight of 18 g/mol.)
Q-8: An aqueous solution containing m moles of non-volatile solute freezes at -0.186oC. Calculate the elevation in the boiling point of the same aqueous solution (Kf = 1.86, Kb= 0.512)
Q-9: What effect does pressure have on the solubility of solids and liquids?
Q-10: In the following pairs, identify the most important type of intermolecular attractive interaction:
(a) n-hexane and n-pentane
(b) I2 and CCl4
(c) NaClO4 and water
Q-11: What is the nature of molecular interactions in solutions with positive deviations? How does the vapour pressure of such solutions vary?
Q-12: Which of the following will form a non-ideal solution?
- C2H5OH + water
- HNO3 + water
- CHCl3 + CH3COCH3
- C6H6 and C6H5CH3
Q-13: Which of the following pairs of solutions does not have the same van’t Hoff factor value?
a) 0.10 M FeSO4 and 0.05 M K4[Fe(CN)6]
b) 0.10 M K4[Fe(CN)6] and 0.05 M FeSO4(NH4)2SO4.6H2O
c) 0.20 M NaCl and 0.10 M BaCl2
d) 0.05 M FeSO4(NH4)2SO4.6H2O and 0.02 M KCl.MgCl2.6H2O
Q-14: A plot of osmotic pressure against concentration(gL-1) of a polymer is constructed. The slope of the plot
a) increases with increase in temperature
b) increases with increase in molar mass of polymer
c) decreases with decrease in concentration of the polymer
d) decreases with increase in temperature
Q-15: Calculate the freezing point (in oC) of 0.1 g of K3[Fe(CN)6](mol. Wt. 329) in 100 g of water (Kf= 1.86 K Kg/mol)
Q-16:
a)Define Henry’s law.
b) How is the KH value related to the solubility of gases in the liquid?
Q-17: Give an example of a compound where hydrogen bonding results in dimer formation.
Q-18: Which of M and m is a better concentration term, and why?
Q-19: Which colligative property is preferred for determining the molar mass of macromolecules?
Q-20: According to Reema, a class XII Chemistry student, normal saline solution containing 0.9 percent (mass/volume) NaCl is isotonic with the fluid inside the cell.As a result, injecting normal saline solution intravenously is risk-free.
(a)Define Isotonic solutions. What happens if the saline solution concentration is (i) greater, (ii) less than 0.9 percent (mass/volume) NaCl?
(b) What values are associated with Reema’s statement?
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