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Chapters
▶ 2: Solutions
3: Ionic Equilibria
4: Chemical Thermodynamics
5: Electrochemistry
6: Chemical Kinetics
7: Elements of Groups 16, 17 and 18
8: Transition and Inner transition Elements
9: Coordination Compounds
10: Halogen Derivatives
11: Alcohols, Phenols and Ethers
12: Aldehydes, Ketones and Carboxylic acids
13: Amines
14: Biomolecules
15: Introduction to Polymer Chemistry
16: Green Chemistry and Nanochemistry
![Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 2 - Solutions - Shaalaa.com](/images/chemistry-english-12-standard-hsc_6:74400b801d4c44ef8e058ff9d9dfe964.jpg "Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 2 - Solutions")
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Solutions for Chapter 2: Solutions
Below listed, you can find solutions for Chapter 2 of Maharashtra State Board Balbharati for Chemistry [English] 12 Standard HSC.
Balbharati solutions for Chemistry [English] 12 Standard HSC 2 Solutions Exercises [Pages 44 - 46]
Choose the most correct option.
The vapour pressure of a solution containing 2 moles of a solute in 2 moles of water (vapour pressure of pure water = 24 mm Hg) is ______.
24 mm Hg
32 mm Hg
48 mm Hg
12 mm Hg
Choose the most correct option.
The colligative property of a solution is _______.
vapour pressure
boiling point
osmotic pressure
freezing point
Choose the most correct option.
In calculating osmotic pressure the concentration of solute is expressed in _______.
molarity
molality
mole fraction
mass percent
Choose the most correct option.
Ebullioscopic constant is the boiling point elevation when the concentration of a solution is _______.
1 m
1 M
1 mass %
1-mole fraction of solute.
Choose the most correct option.
Cryoscopic constant depends on _______.
nature of solvent
nature of solute
nature of solution
number of solvent molecules
Identify the CORRECT statement.
Vapour pressure of solution is higher than that of pure solvent.
Boiling point of solvent is lower than that of solution.
Osmotic pressure of solution is lower than that of solvent.
Osmosis is a colligative property.
Choose the most correct option.
A living cell contains a solution which is isotonic with 0.3 M sugar solution. What osmotic pressure develops when the cell is placed in 0.1 M KCl solution at body temperature?
5.08 atm
2.54 atm
4.92 atm
2.46 atm
Choose the most correct option.
The osmotic pressure of blood is 7.65 atm at 310 K. An aqueous solution of glucose isotonic with blood has the percentage (by volume)________.
5.41 %
3.54 %
4.53 %
53.4 %
Choose the most correct option.
Vapour pressure of a solution is _______.
directly proportional to the mole fraction of the solute
inversely proportional to the mole fraction of the solute
inversely proportional to the mole fraction of the solvent
directly proportional to the mole fraction of the solvent
Choose the most correct option.
Pressure cooker reduces cooking time for food because _______.
boiling point of water involved in cooking is increased
heat is more evenly distributed in the cooking space
the higher pressure inside the cooker crushes the food material
cooking involves chemical changes helped by a rise temperature
Choose the most correct option.
Henry’s law constant for a gas CH3Br is 0.159 mol dm-3 atm-1 at 25 °C. What is the solubility of CH3Br in water at 25 °C and partial pressure of 0.164 atm?
0.0159 mol L-1
0.164 mol L-1
0.026 M
0.042 M
Choose the most correct option.
Which of the following statement is NOT correct for 0.1 M urea solution and 0.05 M sucrose solution?
Osmotic pressure exhibited by urea solution is higher than that exhibited by sucrose solution
Urea solution is hypertonic to sucrose solution
They are isotonic solutions
Sucrose solution is hypotonic to urea solution
Answer the following in one or two sentences.
What is osmotic pressure?
Answer the following in one or two sentences.
A solution concentration is expressed in molarity and not in molality while considering osmotic pressure. Why?
Answer the following in one or two sentences.
Write the equation relating boiling point elevation to the concentration of the solution.
Answer the following in one or two sentences.
A 0.1 m solution of K2SO4 in water has a freezing point of –4.3°C. What is the value of van’t Hoff factor if Kf for water is 1.86 K kg mol–1?
Answer the following in one or two sentences.
What is van’t Hoff factor?
Answer the following in one or two sentences.
How is van’t Hoff factor related to degree of ionization?
Answer the following in one or two sentences.
Which of the following solution will have higher freezing point depression and why?
i. 0.1 m NaCl
ii. 0.05 m Al2(SO4)3
Answer the following in one or two sentences.
State Raoult’s law for a solution containing a nonvolatile solute.
Answer the following in one or two sentences.
What is the effect on the boiling point of water if 1 mole of methyl alcohol is added to 1 dm3 of water? Why?
Answer the following in one or two sentences.
Which of the four colligative properties is most often used for molecular mass determination? Why?
Answer the following.
How vapour pressure lowering is related to a rise in the boiling point of solution?
Answer the following.
What are isotonic and hypertonic solutions?
Answer the following.
A solvent and its solution containing a nonvolatile solute are separated by a semipermeable membrane. Does the flow of solvent occur in both directions? Comment giving a reason.
Answer the following.
The osmotic pressure of CaCl2 and urea solutions of the same concentration at the same temperature are respectively 0.605 atm and 0.245 atm, calculate van’t Hoff factor for CaCl2.
Answer the following.
Explain reverse osmosis.
Answer the following.
How molar mass of a solute is determined by osmotic pressure measurement?
Answer the following.
Why vapour pressure of a solvent is lowered by dissolving a nonvolatile solute into it?
Answer the following.
Using Raoult’s law, how will you show that ΔP = `"P"_1^0 "x"_2`? Where, x2 is the mole fraction of solute in the solution and `"P"_1^0` vapour pressure of pure solvent.
Answer the following.
While considering boiling point elevation and freezing point depression a solution concentration is expressed in molality and not in molarity. Why?
Derive the relationship between the degree of dissociation of an electrolyte and van’t Hoff factor.
What is the effect of temperature on solubility of solids in water? Give examples.
Obtain the relationship between freezing point depression of a solution containing nonvolatile-nonelectrolyte solute and its molar mass.
Explain with diagram the boiling point elevation in terms of vapour pressure lowering.
Fish generally needs O2 concentration in water at least 3.8 mg/L for survival. What partial pressure of O2 above the water is needed for the survival of fish? Given the solubility of O2 in water at 0 °C and 1 atm-1 partial pressure is 2.2 × 10-3 atm mol/L.
The vapour pressure of water at 20°C is 17 mm Hg. What is the vapour pressure of solution containing 2.8 g urea in 50 g of water?
A 5% aqueous solution (by mass) of cane sugar (molar mass 342 g mol-1) has a freezing point of 271 K. Calculate the freezing point of 5% aqueous glucose solution.
A solution of citric acid C6H8O7 in 50 g of acetic acid has a boiling point elevation of 1.76 K. If Kb for acetic acid is 3.07 K kg mol-1, what is the molality of solution?
An aqueous solution of a certain organic compound has a density of 1.063 g mL-1 , osmotic pressure of 12.16 atm at 25 °C and a freezing point of 1.03 °C. What is the molar mass of the compound?
A mixture of benzene and toluene contains 30% by mass of toluene. At 30 °C, vapour pressure of pure toluene is 36.7 mm Hg and that of pure benzene is 118.2 mm Hg. Assuming that the two liquids form ideal solutions, calculate the total pressure and partial pressure of each constituent above the solution at 30 °C.
At 25 °C, a 0.1 molal solution of CH3COOH is 1.35 % dissociated in an aqueous solution. Calculate the freezing point and osmotic pressure of the solution assuming molality and molarity to be identical.
A 0.15 m aqueous solution of KCl freezes at - 0.510 °C. Calculate i and osmotic pressure at 0 °C. Assume the volume of solution equal to that of water.
Solutions for 2: Solutions
Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 2 - Solutions
Shaalaa.com has the Maharashtra State Board Mathematics Chemistry [English] 12 Standard HSC Maharashtra State Board solutions in a manner that help students grasp basic concepts better and faster. The detailed, step-by-step solutions will help you understand the concepts better and clarify any confusion. Balbharati solutions for Mathematics Chemistry [English] 12 Standard HSC Maharashtra State Board 2 (Solutions) include all questions with answers and detailed explanations. This will clear students' doubts about questions and improve their application skills while preparing for board exams.
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Concepts covered in Chemistry [English] 12 Standard HSC chapter 2 Solutions are Solutions, Types of Solutions, Capacity of Solution to Dissolve Solute, Solubility, Vapour Pressure of Solutions of Liquids in Liquids, Colligative Properties of Nonelectrolyte Solutions, Vapour Pressure Lowering, Boiling Point Elevation, Depression in Freezing Point, Osmosis and Osmotic Pressure, Colligative Properties of Electrolytes.
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