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question_answer1) Define (i) solute and (ii) solvent.
question_answer2) Is smoke a homogeneous solution?
question_answer3) Oil and water don't mix. Why?
question_answer4) How is that alcohol and water are miscible in all proportions?
question_answer5) is soluble in water but not in benzene. Why?
question_answer6) Benzene is soluble in toluene but not in water. Why?
question_answer7) Which concentration term remains unaffected by temperature?
question_answer8) Why does the molality of solution remain unchanged with temperature?
question_answer9) Why is molality preferred over molarity of solution?
question_answer10) How does molarity of solution change with temperature?
question_answer11) Explain the term "mole fraction".
question_answer12) Why are soda water and soft drink bottles sealed under pressure?
question_answer13) State Henry's law about the solubility of gases in a liquid.
question_answer14) Why is vapour pressure of solution of glucose in water lower than that of pure water?
question_answer15) State Raoult's law of vapour pressure.
question_answer16) Name two factors on which the vapour pressure of the liquid depends.
question_answer17) Define Raoult's law of solutions containing volatile components.
question_answer18) Define an ideal solution.
question_answer19) What is enthalpy change and volume change when an ideal solution is formed?
question_answer20) State any two characteristics of ideal solutions.
question_answer21) Give an example of ideal solution.
question_answer22) What are the sign of and for a solution with positive deviation from ideal behaviour ?
question_answer23) What are the sign of and for a solution with negative deviation from ideal behaviour?
question_answer24) Give an example of solution showing negative deviation from ideal behaviour.
question_answer25) Give an example of solution showing positive deviation from ideal behaviour.
question_answer26) What type of solution is formed when chloroform is mixed with acetone?
question_answer27) What type of solution is formed when ethahol is mixed with water?
question_answer28) Give an example of solution which shows negative deviation from ideality.
question_answer29) Give an example of solution which shows positive deviation from ideality.
question_answer30) Define azeotropic mixture.
question_answer31) What are maximum boiling azeotropes? Give an example,
question_answer32) What are minimum boiling azeotropes? Give an example.
question_answer33) What type of behaviour is expected when water is added to sulphuric acid?
question_answer34) What is an antifreeze?
question_answer35) Define "colligative properties".
question_answer36) Why does the boiling point of a solution increase on adding non-volatile solute?
question_answer37) Why does the freezing of a solution decrease on adding non-volatile solute?
question_answer38) On what factor does the elevation in boiling point depend?;
question_answer39) On what factors does depression in freezing point depend?'.
question_answer40) How does the boiling point of a liquid change with external pressure?
question_answer41) What change is observed in boiling point of a liquid at higher altitude?
question_answer42) Define cryoscopic constant.
question_answer43) Define ebullioscopic constant.
question_answer44) What is osmosis?
question_answer45) Define osmotic pressure.
question_answer46) State how does osmotic pressure vary with temperature?
question_answer47) How does osmotic pressure depend upon number of moles of solute particles?
question_answer48) Doctors advise gargles by saline water in case of sore throat Why?
question_answer49) What is reverse osmosis?
question_answer50) What is the-use of reverse osmosis?
question_answer51) What are isotonic solution?
question_answer52) Define (i) Hypertonic solution and (ii) Hypotonic.
question_answer53) What is van't Hoff's factor?
question_answer54) When is the value of van't Hoff factor more than one?
question_answer55) When is the value of van't Hoff factor less than one?
question_answer56) Name the colligative property mostly used for the determination of molecular mass of macromolecules.
question_answer57) Which will have greater boiling point (i) 1 M urea solution and (ii) 1 M NaCI solution.
question_answer58) Osmotic pressure of 1 M KCl solution is higher than 1 M urea solution. Why?
question_answer59) Why a mixture of liquids shows negative deviation from ideal behaviour?
question_answer60) Why a mixture of liquids shows positive deviation from ideal behaviour?
question_answer61) Differentiate between molarity and molality of solution.
question_answer62) Give an example each of miscible liquid pairs showing positive and negative deviations from Raoult's law. Give reasons for each such deviation.
question_answer63) Define vapour pressure. What happens to the vapour pressure when (i) volatile solute dissolves in the liquid, (ii) non-volatile solute dissolves in the liquid.
question_answer64) With suitable diagram and appropriate examples explain a non-ideal solution with +ve deviation.
question_answer65) With suitable diagram and appropriate examples explain a non-ideal solution with -ve deviation.
question_answer66) Show graphically how the vapour pressure of a solvent and a solution of non-volatile solute in it change with temperature.
question_answer67) IIIustrate elevation in boiling point with the help of vapour pressure, temperature curve of a solution. Show that elevation in boiling point is a colligative property.
question_answer68) Explain why freezing point of a solvent is lowered on dissolving a non-volatile solute in it. Give an important application of freezing point depression.
question_answer69) IIIustrate depression in freezing point of a liquid when a non-volatile solute is dissolved in it.
question_answer70) Why dried fruits and vegetables slowly swell when placed in water? What will be the effect of temperature this process?
question_answer71) Define osmosis and osmotic pressure.
question_answer72) (i) What is osmotic pressure and how is it related with the molecular mass of the non-volatile solution? (ii) What is the advantage of osmotic pressure method over boiling point elevation method for determining molecular masses?
question_answer73) What is meant by abnormal molecular mass of solute? Which factor is responsible for abnormality in molecular masses of solutes using colligative properties?
question_answer74) The molecular mass of ethanoic acid when determined by colligative property of its solution is abnormal. Explain why?
question_answer75) Explain with suitable examples in each case why the molar masses of some substances determined with the help of colligative properties are (i) higher (ii) lower than the actual values.
question_answer76) (a) What is solubility of a substance? (b) On what factors solubility of solid depends? (c) What is the effect of pressure on solubility?
question_answer77) (a) Define vapour pressure. (b) State and explain Raoult's law for a solution of volatile liquids. (c) State Raoult's law for a solution of non-volatile solute.
question_answer78) What are ideal and non-ideal solutions? Explain each with diagram and suitable examples.
question_answer79) Explain the terms : (a) Elevation in boiling point. (b) Depression in freezing point. (c) Relative lowering of vapour pressure. (d) Osmotic pressure.
question_answer80) What is van't -Hoff factor? How is it used to calculate molecular mass of a non-volatile substances?
question_answer81) What happens when RBC are placed in (i) 1% NaCI solution. (ii) Pure water.
question_answer82) 4% NaOH solution (mass/volume) and 6% urea solution (mass/volume) are equimolar but not isotonic. Why?
question_answer83) Name the solid that is separated when salt solution is slowly frozen.
question_answer84) Why do aquatic species feel more comfortable in winter than in summer?
question_answer85) What precaution should be taken in intravenous injection?
question_answer86) Why is camphor preferred solvent in the determination of molecular mass of non-volatile solute by cryoscopic method (Rast method)?
question_answer87) What happens to the colligative properties when is added to aqueous solution of KI?
question_answer88) A mixture of ethyl alcohol and water cannot be separated into pure component by fractional distillation. Why?
question_answer89) Give one example of interstitial and substitutional solid solutions.
question_answer90) How is Henry's Law constant related to the solubility of a gas in a solvent?
question_answer91) How can you compare the relative solubilities of different salts in the same solvent?
question_answer92) What does normality (N) represent?
question_answer93) Why does not molality of the solution change with temperature?
question_answer94) What are the units of mole fraction?
question_answer95) What should be the nature of the solution while representing the solubility of a solute?
question_answer96) Rubbing isopropyl alcohol often gives a cooling sensation to the skin. Why?
question_answer97) What will happen to the boiling point of the solution on mixing two miscible liquids showing negative deviation from Raoult's law?
question_answer98) The bottle of liquid ammonia is generally cooled before opening the seal. Assign reason.
question_answer99) Does osmosis occur from hypertonic solution to hypotonic solution?
question_answer100) What type of azeotrope will result on mixing chloroform and acetone?
question_answer101) Name the most commonly used semi permeable membrane in the laboratory.
question_answer102) The Van't Hoff factor of a solution is 1. What does it indicate?
question_answer103) What is the purpose of adding ethylene glycol to water?
question_answer104) Why does the solubility of \[NaCl\] in water increase with the rise in temperature?
question_answer105) What is the effect of temperature on the molarity of a solution?
question_answer106) Can a solution of its own have osmotic pressure?
question_answer107) Two liquids A and B upon mixing form a warm solution. What type of deviations do they show from Raoult's Law?
question_answer108) What will happen when red blood corpuscles (RBCs) are placed in (a) 1 % NaCI solution (b) 0.6% NaCI solution?
question_answer109) What should be the maximum concentration of the solute in case a solution is to be ideal?
question_answer110) What will the nature of the solid solution formed on mixing two solids with large difference in particle size?
question_answer111) Which colligative property is generally used for determining the molar mass of a solute?
question_answer112) What is common in all the four colligative properties?
question_answer113) Will osmosis take place when 0.1 M aqueous urea and glucose solutions are separated by semi permeable membrane?
question_answer114) The cryoscopic constant \[({{K}_{f}})\] for water is \[1.86\,\,K\,mo{{l}^{-1}}\,k{{g}^{-1}}\]. What does it signify?
question_answer115) How does osmotic pressure depend upon temperature?
question_answer116) Which aqueous solution has higher concentration ; 1 molar or 1 molal having the same solute?
question_answer117) Why is molality of a solution preferred for expressing concentration over molarity?
question_answer118) Will elevation in boiling point temperature be same for \[0\cdot 1M\]NaCI and \[0\cdot 1M\]sucrose solution?
question_answer119) What is the expected deviation from ideal solution behaviour when acetone and chloroform are mixed to form a solution?
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