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Chemistry - Ionic Equilibrium

Practise 102 NTA Abhyas (JEE Main) questions on Ionic Equilibrium. Each question shows a quick preview so you can jump straight to the topic you want to revise.

Ionic Equilibrium has been asked in 0 of the 25 years of NTA Abhyas (JEE Main) papers analysed (2002–2026), with 102 questions in all. 100% of them were easy, 0% moderate and 0% tough. Most of its questions came from 2026, with 0 questions that year. In the last three years (2024–2026) it had 0 questions across 49 papers, about 0 per paper.

All of the chapter's questions come from a single topic, Uncategorized.

  1. 1Find out the percentage dissociation of an acid having conc. of 10 M and dissociation constant 1.0 × 1 0 - 3 .
  2. 2Calculate pH at which an acid indicator HIn with concentration 0.1 M changes its colour ( K a for HIn = 1 × 1 0 - 5 ).
  3. 3K a for HCN is 5 x 10 - 10 at 25 o C. For maintaining a constant pH of 9, the volume of 5 M KCN solution required to be added to 10 mL of 2
  4. 4The pH of 0.1 M solution of a weak acid H A is 4.50. It is neutralised with certain ammount of N a O H solution to decrease the acid content
  5. 5Silver ions are added to the solution with Br − = Cl − = CO 3 2 − = AsO 4 3 − = 0 .1 M Which compound will precipitate at the lowest [ A g +
  6. 6Which one of the following mixture does not act as a buffer solution-
  7. 7The Solubility of A B 2 is 0 .05 g per 100 mL at 25 o C . Calculate K sp of A B 2 at 25 o C? [Atomic mass of A = 20 amu, atomic mass of B =
  8. 8The ionization constant of a weak monobasic acid is 25 × 1 0 – 6 while the equivalent conductance of its 0.01 M solution is 19.6 S c m 2 e q
  9. 9If the pK a of a weak acid HA is 4 .80 and the pK b of a weak base BOH is 4 .78 . Then, the pH of an aqueous solution of the corresponding s
  10. 10For H 2 S ; K a 1 = 10 - 7 , K a 2 = 1 0 - 1 4 . A Saturated solution of H 2 S in 0.1 M H 2 S contains Mn 2 + , Co 2 + and Ag + at an origin
  11. 11How many among the following species can be classified as Lewis acids? CH 3 ⊕ , C l ⊕ , CO 2 , CCl 2 , BCl 3 , BI 3 , Fe + 2 , AlCl 3
  12. 12An acid base indicator has K a = 3 × 1 0 - 5 . The acid form of the indicator is red and the basic form is blue. By how much must the pH cha
  13. 13If 200 mL of a 0 .031 molar solution of H 2 SO 4 are added to 84 mL of a 0 .150 M KOH solution, what is the pH of the resulting solution?
  14. 14p H of a 1000 c c solution is 2 . It will not change if
  15. 15For the indicator, HIn; the ratio In - HIn is 7 .0 at pH of 4 .3 . K In for the indicator is [ Given: log 7 = 0 .845 and Antilog ( − 3.455 )
  16. 16The pH of 0.1 (M) solution of the following salts increases in the order
  17. 17Calculate the number of moles of N H 4 C l that should be added to one litre of 1.0 M N H 4 O H to prepare buffer solution with pH = 9 K b =
  18. 18Bromine in excess is dropped to a 0.01 M SO 2 . All of SO 2 is oxidized to H 2 SO 4 and the excess Br 2 is removed by flushing with gaseous
  19. 19Match List I with List II and select the correct answer using codes given below the lists. List I List II ( p ) Potassium sulphate 1 . Acidi
  20. 20The equilibrium constant for : CN - + CH 3 COOH ⇌ HCN + CH 3 COO - is : ( G i v e n p K b f o r C N - = 4.69 a n d p K b f o r C H 3 C O O -
  21. 21The solubility of a sparingly soluble salt A OH 2 (mol. wt. 192.3) is 19 .23 g / litre at 300 K . The pH of its saturated solution assuming
  22. 22Three sparingly soluble salts that have same solubility products as given below I. A 2 X II. A X III. A 2 X 3 Their solubilities in a satura
  23. 23The K sp of FeS = 4 × 10 − 19 at 298 K . The minimum concentration of H + ions required to prevent the precipitation of FeS from a 0 .01 M s
  24. 24The pH of blood stream is maintained by a proper balance of H 2 C O 3 and N a H C O 3 concentration. What volume of 5 M N a H C O 3 solution
  25. 25The degree of dissociation of acetic acid in a 0 .1 M solution is 1.0 × 1 0 – 2 . The p K a of acetic acid value.
  26. 26What will be the pH of a solution formed by mixing 40 c m 3 of 0.1 M HCl with 10 c m 3 of 0.45 M NaOH?
  27. 27What will be the pH of a solution formed by mixing 10 mL 0.1 M N a H 2 P O 4 and 15 mL 0.1 M N a 2 H P O 4 ? [Given: for H 3 PO 4 p K a 1 =
  28. 28K a for HCN is 5 × 1 0 - 10 at 25 ° C . For maintaining a constant pH of 9, the volume in ml of 5 M KCN solution required to be added to 10
  29. 29One litre of 1 M solution of an acid HA K a = 10 − 4 at 25 o C has pH = 2 . It is diluted by water so the new p H becomes double. The soluti
  30. 30At 25 ° C the p H of a 10 – 8 M H C l solution in water is
  31. 31If the pK a of acetic acid and pK b of NH 4 OH are 4.76 and 4.75 respectively, what will be the pH of ammonium acetate solution?
  32. 32How many litres of water must be added to 1 litre an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2?
  33. 33Calcium lactate is a salt of weak acid i.e., lactic acid having general formula C a ( L a C ) 2 . Aqueous solution of salt has 0.3 M concent
  34. 34Arrange in increasing order of solubility of AgBr in solutions given here (i) 0.1 M N H 3 (ii) 0.1 M A g N O 3 (iii) 0.2 M NaBr (iv) pure wa
  35. 35Calculate dissociation constant for an acid HA having [ H + ] equals to 0 .1 M (Given: degree of dissociation of HA is 1% )
  36. 36The increasing order of Ag + ion concentration in I. Saturated solution of AgCl II. Saturated solution of Agl III. 1 M Ag NH 3 2 + in 0.1 M
  37. 374 ml of HCl solution of pH = 2 is mixed with 6 ml of NaOH solution of pH = 12. What would be the final pH of solution? (log 2 = 0.3)
  38. 38What is H + in a solution that is 0.01 M in H C N and 0.02 M in NaCN? br /> ( K a for H C N = 6.2 × 1 0 - 10 )
  39. 39Solid N a 2 S O 4 is slowly added to a solution which is 0.020 M in B a N O 3 2 and 0.020 M in P b N O 3 2 . Assume that there is no increas
  40. 40HX is a weak acid K a = 1 0 - 5 . It forms a salt NaX [0.1 M (aq)] on reacting with aqueous caustic soda solution. The percentage of hydroly
  41. 410 .1 M NaOH is titrated with 0 .1 M, 20 ml HA till the end point, K a HA = 6×10 − 6 and degree of dissociation of HA is small as compared to
  42. 42Calculate H + and % dissociation of 0.1 M solution of N H 4 O H solution. The ionisation constant for N H 4 O H is k b = 2.0 × 1 0 - 5
  43. 43An aqueous solution contains an unknown concentration of B a 2 + . When 50 mL of a 1 M solution of N a 2 S O 4 is added B a S O 4 just begin
  44. 44In a buffer solution having equal concentrations of B - and HB the value of K b for B - is 1 0 - 9 . The pH of buffer solution is
  45. 45The pH of 0.1 M solution of the following salts increases in the order
  46. 46Calculate the p H of solution when 100 m L , 0.1 M C H 3 C O O H and 100 m L , 0.1 M H C O O H are mixed together. (Given: K a C H 3 C O O H
  47. 47If pH of a saturated solution of Ba OH 2 is 12 , the value of its K ( sp ) is found to be n × 1 0 - 7 M 3 . find the value of ‘ n ’ here?
  48. 48A g B r ( s ) + 2 S 2 O 3 2 - ( a q ) ⇌ A g ( S 2 O 3 ) 2 3 - ( a q ) + B r - ( a q ) Given K s p ( A g B r ) = 5 × 1 0 - 13 ; K f A g ( S 2
  49. 49K b for CH 2 ClCOO - is 6.4 × 10 - 12 . The pH of 0.1 M CH 2 ClCOONa in water is :
  50. 50The simultaneous solubility of AgCN K s p = 2.5 × 1 0 - 6 and AgCl K s p = 1.6 × 1 0 - 10 in 1 M N H 3 (aq) are respectively Given K f [ A g

Frequently Asked Questions

1.How many questions are available for Ionic Equilibrium?

This chapter includes 102 NTA Abhyas (JEE Main) questions.

2.Are these questions only from NTA Abhyas (JEE Main), or from other exams too?

These are NTA Abhyas (JEE Main) questions specifically for the Ionic Equilibrium chapter. Questions from other exams like JEE Main or JEE Advanced are organised separately under their respective exam sections.

3.What is the difficulty level of Ionic Equilibrium questions in NTA Abhyas (JEE Main)?

Of the 102 questions analysed for this chapter, 100% are easy, 0% moderate and 0% tough. 2026 had the most, with 0 questions.

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

All of this chapter's questions come from a single topic: Uncategorized.