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Chemistry - Ionic Equilibrium

Practise 47 AIIMS previous year questions on Ionic Equilibrium, compiled from papers spanning 2001 to 2019. Each question is pulled directly from the actual exam paper it appeared in, so you're practising in the exact style and difficulty AIIMS tests.

Ionic Equilibrium has been asked in 19 of the 19 years of AIIMS papers analysed (2001–2019), with 47 questions in all. 32% of them were easy, 32% moderate and 36% tough. Most of its questions came from 2001, with 7 questions that year. In the last three years (2017–2019) it had 7 questions across 5 papers, about 1.4 per paper.

The chapter's 6 topics are not weighted equally: PH of solutions (18 questions, 38%), Solubility (11 questions, 23%), and Salt Hydrolysis (7 questions, 15%) have been asked the most. PH of solutions has produced the most tough questions (8).

  1. 1Assertion : Some salts are sparingly soluble in water at room temperature. Reason : The entropy increases on dissolving the salts.26 May, 2019Solubility
  2. 2Which of the following has maximum solubility at low ?25 May, 2019PH of solutions
  3. 3Calculate ionisation constant for pyridinium hydrogen chloride. (Given that ion concentration is and its concentration is .)27 May, 2018Salt Hydrolysis
  4. 4When of is mixed with of then what is the of resultant solution?26 May, 2018PH of solutions
  5. 5Calculate the overall complex dissociation equilibrium constant for the ions, given that stability constant for this complex is .2017Theories of Acids and Bases
  6. 6is white when cold and yellow when heated. It is due to the development of2017Salt Hydrolysis
  7. 7for is at . For maintaining a constant , the volume of solution required to be added to of solution is2017PH of solutions
  8. 8for the reaction is 4 . If initially only is present then what will be the partial pressure of after equilibrium?2016Solubility
  9. 9Assertion : is stronger acid than . Reason : is more electronegative than , conjugate base is more stable than .2016Theories of Acids and Bases
  10. 10The pair of amphoteric hydroxides is2015Ionic Product of Water
  11. 11Assertion: is not soluble in yellow ammonium sulphide. Reason : The common ion effect due to ions reduces the solubility of .2015Solubility
  12. 12Assertion: Mixture of and is an example of acidic buffer. Reason: Acidic buffer contains equimolar mixture of weak acid and its salt with we2014Buffer solutions
  13. 13What will be the solubility product of ?2013Solubility
  14. 14Which has the highest ?2012PH of solutions
  15. 15The compound which does not exist as hydrate form2011Salt Hydrolysis
  16. 16of is , find the volume for of (M.wt. = 136).2011Solubility
  17. 17is neutralised by of . Then of resulting solution is2011PH of solutions
  18. 18What is the of glycine solution? For glycine and at .2010PH of solutions
  19. 19The standard half-cell reduction potential for is at . Given the experimental value for , calculate the standard half-cell reduction potenti2010Solubility
  20. 20of a solution2009PH of solutions
  21. 21Formula of microcosmic salt is2009Salt Hydrolysis
  22. 22The correct order of increasing \( [ {H}_3 {O}^{+} ]\)in the following aqueous solutions is2008PH of solutions
  23. 23The \( {pH}\) of the solution obtained on neutralisation of \(40 {~mL~} 0.1 {~M~} {NaOH}\) with \(40 {~mL~} 0.1 {~M~} {CH}_3 {COOH}\) is2007PH of solutions
  24. 24During titration of acetic acid with aq. \( {NaOH}\) solution, the neutralisation graph has a vertical line. This line indicates2007Salt Hydrolysis
  25. 25Assertion : Mixture of \( {CH}_3 {COOH}\) and \( {CH}_3 {COONH}_4\) is an example of acidic buffer. Reason : Acidic buffer contains equimola2007Buffer solutions
  26. 26of ammonia solution is mixed with of . What is the of the mixture? ( of ammonia solution is 4.74)2006PH of solutions
  27. 27Assertion : is not soluble in yellow ammonium sulphide. Reason : The common ion effect due to ions reduces the solubility of .2006Theories of Acids and Bases
  28. 28When of acetic acid is titrated against of ammonia solution ( ), the equivalence point occurs at2005Salt Hydrolysis
  29. 29Assertion : Addition of to an aqueous solution of in the presence of (excess) precipitates . Reason : is insoluble in water.2005Solubility
  30. 30Dimethyl glyoxime gives a red precipitate with , which is used for its detection. To get this precipitate readily the best range is2004PH of solutions
  31. 31Among the following the dissociation constant is highest for2004Theories of Acids and Bases
  32. 32What is the of glycine solution? For glycine, and at ?2004PH of solutions
  33. 33Assertion : (III) is not precipitated as sulphide when in its alkaline solution is passed. Reason : The concentration of ion in alkaline med2004Solubility
  34. 34Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate rather than .2004Solubility
  35. 35Which one of the following is not a buffer solution?2003Buffer solutions
  36. 36In which of the following acid-base titration, is greater than 8 at equivalence point?2003PH of solutions
  37. 37Assertion : is more soluble in than in plain water. Reason : Carbonate is a weak base and reacts with the from the strong acid, causing the 2003Solubility
  38. 38At , distilled water has ions concentration equal to litre. The value of at this temperature will be2002Ionic Product of Water
  39. 39The of solution containing sodium acetate and acetic acid is for2002Salt Hydrolysis
  40. 40The solubility of is at . The value for is2002Solubility
  41. 41Which of the following is strongest Bronsted base?2001Theories of Acids and Bases
  42. 42When the temperature of reactions will increase then the effect on value will2001PH of solutions
  43. 43The of aqueous solution of ammonium formate is of and of2001PH of solutions
  44. 44The value of decinormal solution of which is ionised is2001PH of solutions
  45. 45The aqueous solution of which of the following salt will have the lowest ?2001PH of solutions
  46. 46A solution with is more acidic than one with a , by a factor of2001PH of solutions
  47. 47Assertion : Relative strength of acids can be known by knowing the value of dissociation constant. Reason : It gives the value of dissolved 2001Ionic Product of Water

Frequently Asked Questions

1.How many questions are available for Ionic Equilibrium?

This chapter includes 47 questions compiled from AIIMS papers spanning 2001 to 2019.

2.Are these questions only from AIIMS, or from other exams too?

These are AIIMS questions specifically for the Ionic Equilibrium chapter. Questions from other exams like NEET or JIPMER are organised separately under their respective exam sections.

3.Is Ionic Equilibrium an important chapter for AIIMS Chemistry?

Ionic Equilibrium has appeared in 19 of the 19 years of AIIMS papers covered here, with 47 questions across 21 papers - about 2 per paper it appears in.

4.What is the difficulty level of Ionic Equilibrium questions in AIIMS?

Of the 47 questions analysed for this chapter, 32% are easy, 32% moderate and 36% tough. 2001 had the most, with 7 questions.

5.Which topics in Ionic Equilibrium should I focus on?

These topics have carried the most weightage in Ionic Equilibrium:

  • PH of solutions - 18 questions (38%)
  • Solubility - 11 questions (23%)
  • Salt Hydrolysis - 7 questions (15%)
  • PH of solutions has produced the most tough questions (8).
6.Is Ionic Equilibrium's weightage in AIIMS going up or down?

Across all 21 papers analysed, Ionic Equilibrium has averaged about 2.2 questions per paper. In the last three years (2017–2019), that average has fallen, at about 1.4 questions per paper. Use the year-wise numbers on this page for the exact trend before you decide how much time to give it.