12th Chemistry 1 Marks Organic nitrogen compounds:

12th Chemistry Important Questions Unit 8 Ionic Equilibrium

12th Chemistry Important Questions Unit 8 Ionic Equilibrium

TN 12th Chemistry Important Questions Unit 8 Ionic Equilibrium. 12th Chemistry Important Questions Chapter 8 Transition And Inner Transition Elements +2 Chemistry Important 2 Marks, 12th Chemistry Important 3 Marks, Chemistry Important 5 Marks Questions Based on reduced Syllabus 2021-2022. 12th Free Online Test (MCQs). HSC 12th Chemistry Revision Test Important Questions. 12th Tamil Full Guide.

12th Chemistry Important Questions Unit 8 Ionic Equilibrium

12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

 

12th Chemistry All Units Important Questions

8. Ionic Equilibrium

  • 1. What are Lewis acids and bases? Give two examples for each.
  • 2. Discuss the Lowry – Bronsted concept of acids and bases.
  • 3. Indentify the conjugate acid base pair for the following reaction in
    i, HS(aq) + HF ⇌ F(aq) + H2S(aq) ii, HPO42- + SO32-⇌ PO43- + HSO4
    iii, NH4+ + CO32- ⇌ NH3 + HCO3
  • 4. Account for the acidic nature of HClO4 in terms of Bronsted – Lowry theory, identify its conjugate base.
  • 5. When aqueous ammonia is added to CuSO4 solution, the solution turns deep blue due to the formation of tetramminecopper (II) complex, [Cu(H2O)4]2+(aq) + 4NH3(aq)⇌ [Cu(NH3)4]2+(aq) + 4H2O, among H2O
    and NH3 Which is stronger Lewis base.
  • 6. The concentration of hydroxide ion in a water sample is found to be 2.5 ×10-6M. Identify the nature of the solution.
  • 7. A lab assistant prepared a solution by adding a calculated quantity of HCl gas at 25oC to get a solution with [H3O+]= 4× 10-5 M. Is the solution neutral (or) acidic (or) basic.
  • 8. Calculate the pH of 0.04 M HNO3Solution.
  • 9. Define solubility product
  • 10. Define ionic product of water. Give its value at room temperature.
  • 11. Explain common ion effect with an example
  • 12. Derive an expression for Ostwald‟s dilution law
  • 13. Define pH
  • 14. Calculate the pH of 1.5×10-3M solution of Ba(OH)2
  • 15. 50ml of 0.05M HNO3 is added to 50ml of 0.025M KOH . Calculate the pH of the resultant solution.
  • 16. The Ka value for HCN is 10-9 . What is the pH of 0.4M HCN solution?
  • 17. Solubility product of Ag2CrO4 is 1×10-12 . What is the solubility of Ag2CrO4 in 0.01M AgNO3 solution?
  • 18. Write the expression for the solubility product of Ca3(PO4)2
  • 19. A saturated solution, prepared by dissolving CaF2(s)in water, has [Ca2+]=3.3× 10-4 M What is the Ksp of CaF2?. Calculate the pH of the resultant solution.
  • 20. Ksp of AgCl is 1.8 ×10−10 . Calculate molar solubility in 1 MAgNO3
  • 21. A particular saturated solution of silver chromate Ag2CrO4 has [Ag+]=5 ×10-5and
    22. [CrO 2-] =4.4 × 10 M What is the value of K for Ag CrO4 ?
  • 23. Write the expression for the solubility product of Hg2Cl2.
  • 24. Ksp of Ag2CrO4 is 1.1 × 10-12 . what is solubility of Ag2CrO4 in 0.1M K2CrO4.
  • 25. Will a precipitate be formed when 0.150 L of 0.1M Pb(NO3)2 and 0.100L of 0.2 M NaCl are mixed? Ksp (PbCl2)=1.2×10-5
  • 26. Ksp of Al(OH)3 is 1×10-15M. At what pH does 1.0 ×10-3M Al3+ precipitate on the addition of buffer of NH4Cl and NH4OH solution?
  • 27. Discuss the Arrhenius concept of acids and bases
  • 28. What are the limitations of Arrhenius concept?
  • 29. What are conjugate acid – base pairs? give one example?
  • 30. Differenciate Lewis acids and Lewis bases?
  • 31. How will you measure the Strength of Acids and Bases?
  • 32. Derive the ionisation constant or dissociation constant of the acid.
  • 33. Define the degree of ionisation or dissociation
  • 34. The dissociation of a CH3COOH is suppressed in the presence of CH3COONa. Give the reason.
  • 35. What are Buffer solution?
  • 36. Mention types of Buffer solution.
  • 37. Explain the Buffer action of the solution.
  • 38. Derive Henderson – Hasselbalch equation
  • 39. Derive the relationship between pH and pOH
  • 40. How will you determined the solubility product from molar solubility?
  • 41. Define Ostwald‟s dilution law
  • 42. How will you determine strength of Acids and Bases?
  • 43. Calculate the pH of 10-7M HCl
  • 44. What are conjugate acid–base pairs? Give example.
  • 45. 0.1M Solution of HF is weak acid. But 5M solution of HF is a stronger acid. Why?
  • 46. The Ka value of HCN is 10-9. What is the pH of 0.4M HCN solution?.
  • 47. Write pH value of the following
    a) Vinegar b) Baking soda c) Black coffee d) Soapy water

12th Chemistry All Units Important Questions

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