# Solutions-Important Questions & Preparation Tips

Aug 22, 2013 16:50 IST

The experts of jagranjosh.com have full confidence that you will not miss any of the questions in the board exam as well as in competitive exams from this chapter if you will keep the following terms / question in your mind while studying

• Intravenous injections are alwaysdissolved in water containing salts at particular ionicconcentrations. Reason

• The technical definition of solution

• Types of solutions and example of emulsion

• When concentration of a solution is expressed in terms Parts per million

• Definition of mole fraction and derivation of formula(unit of mole fraction)

• Numerical based on mole fraction

• Definitions of molality, molarity and normality and also the relationship among all three

• numerical based on molality, molarity and normality (units of all three)

• Calculate the molarity of a solution containing 5 g of NaOH in 450 mLsolution

• Calculate molality of 2.5 g of ethanoic acid (CH3COOH) in 75 g of benzene.

• Calculate the mole fraction of benzene in solution containing 30% bymass in carbon tetrachloride.

• Analysis of effects of temperature and pressure in case of solubility of solid in liquid and solubility of  gas in liquid

• Definition of Henry’s law interms of mole fraction and partial pressure

• Higher thevalue of KH at a given pressure, the lower is the solubilityof the gas in the liquid. Justify the statement

• If N2 gas is bubbled through water at 293 K, how many millimoles of N2 gas would dissolve in 1 litre of water. Assume that N2 exerts a partial pressure of 0.987 bar. Given that Henry’s law constant for N2 at 293 K is 76.48 kbar.

• Define vapour pressure

• Raoult’s law in case of a binary solution(liquid-liquid solution) and numerical based on the formula related to the same case

• Vapour pressure of chloroform (CHCl3) and dichloromethane (CH2Cl2) at 298 K are 200 mm Hg and 415 mm Hg respectively. (i) Calculatethe vapour pressure of the solution prepared by mixing 25.5 g ofCHCl3 and 40 g of CH2Cl2 at 298 K and, (ii) mole fractions of eachcomponent in vapour phase.

• Describe the situation when Raoult’s law becomesa special case of Henry’s law

• What type of solution can be classified into ideal and non ideal solution?

• Definition and important properties of ideal and non ideal solution

• The intermolecular attractive forces between the A-A and B-B arenearly equal to those between A-B, then identify the type of solution(ideal / non ideal)

• Examples of some combination of solution which comes under the ideal and non ideal solution

• If deviation from the Raoult’s law is +ve ,then identify the type of solution

• When a solution is said to be azeotrope?

• Define the term colligative property  and discuss all the colligative properties in detail

• Kb is called Boiling PointElevation Constant or Molal Elevation Constant (EbullioscopicConstant). What is the unit of Kb?

• Kf, which depends on the nature of thesolvent is known as Freezing Point Depression Constant or Molal Depression Constant or Cryoscopic Constant.what is the unit of Kf

• Define osmosis and osmotic pressure

• What is reverse osmosis

• Derive the relation between osmotic pressure, molarity and concentration of the solution at a given temperature.

• What is edema?

• Boiling point of water at 750 mm Hg is 99.63°C. How much sucrose is tobe added to 500 g of water such that it boils at 100°C.

• Concept of abnormal molar mass and introduction of  Van’t Hoff factor

• Relation between Kb, Kf, and osmotic pressure  with Van’t Hoff factor

• If the solubility product of CuS is 6 × 10–16, calculate the maximum molarity ofCuS in aqueous solution.

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