Ch 9 Chemistry Class 11 Notes

• Define phase. Give an example.
• Define solution. Give an example.
• define solvent and solute.
• Define concentration of solution.
• Define dilute solution and concentrated solution. 
• Mention the concentration units of solution. 
• Mention the units showing percentage composition.
• Mention the various types of solution (Any type can come for short question)
• What is percentage weight/weight? Give an example. 
• What is percentage weight/volume? Give an example.
• What is percentage volume/weight? Give an example. 
• What is percentage volume/volume? Give an example.
• Define molarity. Give an example. 
• Define molality. Give an example. 
• Define mole fraction (x). Give an example. 
• Justify that the solubility principle is “like dissolves like”.
• What are completely miscible liquids?
• What are partially miscible liquids?
• What is critical solution temperature or upper consulate temperature?
• What is the difference between ideal and non-ideal solutions? 
• What are continuous solubility curves?
• What is fractional crystallization? How is it carried out?
• Why molal solution is dilute as compared to molar solution? 
• What is ebullioscopic constant?
• What is cryoscopic constant?
• What are the conditions to observe colligative properties?
• What are the parts in assembly of Landsberger’s apparatus?
• Why ethylene glycol is used as an anti-freeze in car radiators?
• Why the relative lowering of vapour pressure is independent of temperature?
• Non-ideal solutions do not obey the Raoult’s law. Why?
• Boiling points of solvents increase due to the presence of solutes. Why?
• Why Beckmann thermometer is used to note the depression of freezing point?
• Why the freezing points are depressed due to presence of solutes?
• Calculate the molarity of a solution containing 9g of glucose in 250 cm3 of solution.
• How molality is independent of temperature but molarity depends on temperature?
• One molal solution of glucose is dilute as compared to one molar solution of glucose. Justify it.
• Relative lowering of vapor pressure is independent of temperature. Justify
• Justify that boiling point of solvents increase due to presence of non- volatile solutes.
• Depression of freezing point is a colligative property. Justify it. 
• Why NaCl and KNO3 are used to lower the melting points of ice?
• Why is the vapor pressure of a solution lesser than vapor pressure of pure solvent?
• Calculate the percentage by weight of NaCl if 2g of it is dissolved in 20g of water.
• What is meant by water of crystallization? Give an example. 
• What are zeotropic and azeotropic mixtures?
• Differentiate between hydration and hydrolysis.
• What are the names of four major parts of apparatus used in Landsberger’s method for elevation of boiling point?
• Why the solubility of glucose into water increases by increasing temperature?
• Give two statements of Raoult’s law.
• Aqueous solution of CuSO4 is acidic in nature. Justify it. 
• Aqueous solution of CH3COONa is basic in nature. 
• Define and explain the following with one example in each case.
• The sum of mole fractions of all the components is always equal to unity for any solution. Justify. 
• Colligative properties are obeyed when the solute is non-electrolyte, and also when the solutions are dilute. Justify.
• The solutions showing positive and negative deviations cannot be fractionally distilled at their specific compositions. Explain it.
• Explain the effect of temperature on phenol-water system.(You may consult how a phenol-water system works for answer)
• What is the physical significance of Kb and Kf of solvents? OR Define ebullioscopic constant and cryoscopic constant with an example.
• Boiling points of the solvents increase due to the presence of solutes. How?
• In summer the antifreeze solutions protect the liquid of the radiator from boiling over. Justify. 
• Freezing points are depressed due to the presence of solutes. Justify. 
• The boiling point of one molal urea solution is 100.52oC but the boiling point of two molal urea solution is less than 101.04oC
• The total volume of the solution by mixing 100 cm3 of water with 100 cm3of alcohol may not be equal to 200 cm3 . Justify it. 
• Non-ideal solutions do not obey the Raoult’s law. Justify. 
• The concentration in terms of molality is independent of temperature but molarity depends upon temperature.