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1st Year Chemistry Short Questions (Chapter 9)

 If you are in 1st year class


And searching for important short questions for your exams preparation than read it out 


Here is some short questions from chapter 9 of 1st year



 

SOLUTIONS AND CONCENTRATION UNITS 


1. Define phase, solution, solute & solvent.


2. What is meant by w/w , w/v, v/w & v/v composition of the solution?


3. How will you prepare 5 % w/v urea solution in water?


4. Define molarity of a solution. How is molarity related to mass of solute?


5. Calculate the molarity of a solution containing 41.4 g of K2CO3 dissolves in 500 cm3 of given solution. Molar mass of K2CO3 is 138 g mol^-1


6. Calculate the molarity of solution containing 4.5 g of NaOH dissolved in 500 cm3 of solution 


7. Define molality. Explain with one example


8. One molal solution is dilute as compared to one molar solution of glucose.(Why a molar solution is more concentrated than a molal solution) 


9. The concentration in term of molality is independent of temperature but molarity depends on temp. Why?


10. One molal solution of urea in water is dilute as compared to one molar solution of urea ,but no. of particles of solute is same. Justify


11. Define mole fraction & its mathematical expression


12. What is ppm solution. Give mathematical expression


TYPES OF SOLUTIONS


13. Why glucose is not soluble in CCl4, but dissolves in water(Why polar substances are soluble in polar solvents)? 


14. Write about phenol water system


15. What is critical solution temperature. Give example 


16. What is conjugate solution? 


17. What are partially miscible solutions. Give examples 


IDEAL & NON-IDEAL SOLUTIONS (RAOULTS 'S LAW) 


18. Give differences b/w ideal & non-ideal solutions


19. Differentiate b/w zeotropic and azeotropic mixture? 


20. Why non-ideal solutions do not obey Roult's law? 


21. What is positive deviation from Roult's law? 


22. Give two definitions of Roult's law. Write their formulas


SOLUBILITY & SOLUBILITY CURVES


23. Define solubility and solubility curves


24. What are continuous and discontinuous solubility curves. Give examples


25. Why Na2SO4.10H2O shows discontinuous solubility curve


COLLIGATIVE PROPERTIES 


26. What are colligative properties. Why are these called so? 


27. Colligative properties are obeved when the solute is non-electrolyte and also when the solutions are dilute. Explain


28. The boiling point of one molar urea solution and one molar sucrose solution is 100.52 °C. Give reason


LOWERING OF VAPOR PRESSURE 


29. What is lowering of vapor pressure? Write mathematical expression


30. Why relative lowering of vapor pressure is independent of temperature


ELEVATION IN BOILING POINT 


31. What is elevation in boiling point 


32. Why the boiling point of the solvent increase due to the presence of non-volatile solutes?


33. How do you justify that in summer the antifreeze solution protects the liquid of the radiator from boiling over?


34. Explain glycol may be used in the radiator of the automobile. Give two aspects of its use


DEPRESSION IN FREEZING POINT 


35. Why freezing point of solution is always less than freezing point of pure solvent


36. How does the depression in freezing point help us to determine the molar mass Ma of solute?


37. Why Beckman thermometer is used to measure depression in freezing point?


38. What is function of outer larger tube in Beckman 's freezing point apparatus ?


39. State Ebullioscopic & Cryoscopy constant? 


40. Why the NaCl & KNO3 are used to lower the melting point of ice? 


41. Give the physical significance of K & Kb 


ENERGETICS OF SOLUTIONS 


42. Aqueous solution of Copper sulphate is acidic in nature. Explain


43. What are hydrates. Give two examples


44. Aqueous solution of Na2CO3 is alkaline in nature. Explain 


45. Aqueous solution of CH3COONa is basic, Justify 


46.Differentiate b/w hydration & hydrolysis



REGARDS : TALHA 



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