NEET PYQ Ionic Equilibrium - Chapter-wise Questions with Solutions

About Ionic Equilibrium PYQs

Ionic Equilibrium has 764 previous year questions in the Quantrex Academy NEET UG Chemistry bank. The 220 questions in this list come from NEET (116), AIIMS (47), MHT CET Medical (34) and 1 other source, spanning 2001 to 2026. Each question opens on its own page with the options, the correct answer and the worked solution where available.

NEET Ionic Equilibrium PYQs with Solutions

About Ionic Equilibrium PYQs

Questions by year (this list)

Ionic Equilibrium questions with solutions

What amount of NaOH should be dissolved in a 500 mL solution, so that the p^H of solution is 12 at 298 K ?

Which of the following buffer solutions is used for precipitation of cations of the III A group?

The degree of dissociation of weak acid is directly proportional to

Which from the following is Lewis base?

The solubility of Fe(OH)_3 is x mole per liter. Find its K_ sp .

The Basic buffer solution is made with 0.1\ M\ NH_4OH and 0.2\ M\ NH_4Cl . If K_b for the base is 1.8 × 10^ -5 , what is the pH of the buffer?

The hydrogen ion concentration of the ocean is about 2 × 10^ -9 \ M . What is the pOH of ocean?

Calculate the dissociation constant of a weak monobasic acid if it is 0.04% dissociated in a 0.01M solution.

Calculate the solubility of AgCl in mol/dm^3 at 25\ ^ ^ ∘ C . Given: K_ sp \ (AgCl) = 1.8 × 10^ -10

A weak monobasic acid is 0.05\ \% dissociated in its solution, find the degree of dissociation.

Solubility of MA_2 type of electrolyte is 0.5 × 10^ -4 \ mol/litre . Then find out k_ sp of electrolyte?

Which of the following aqueous solutions of salts is neutral?

Calculate the amount of NaOH in g/L in a one L solution of it with the pH of 12. (Molar mass of NaOH=40 g/mol)

The solubility of AgBr at 298 K is 2×10^ -7 \ kg/dm^3 . Find the solubility product of AgBr at same temperature. [Molar mass of AgBr=188 g/mol]

Which of the following salts of weak acids and weak bases on hydrolysis turns red litmus blue? [K_a for acetic acid = 1.8×10^ -5 , K_a for hydrofluoric acid = 6.8×10^ -4 , K_a for

What is pH of HCl solution containing 0.365 g of HCl in 100 mL of solution, assuming complete dissociation at 298 K? ( Molar mass of HCl = 36.5 g/mol)

Which from the following is NOT a buffer solution?

Calculate the pH of the buffer solution consists of 0.005 M weak acid and 0.02 M of its salt with strong base BA. [ pK_a = 3.4437 ]

The solubility product of Ag_2CrO_4 is 4 × 10^ -12 . What is the amount of Ag_2CrO_4 in gram present in 100 ml its saturated solution? (molar mass of Ag_2CrO_4 = 331.73 g/mol).

The pH of HCl and H_2SO_4 is same at same temperature. What is the ratio of molar concentration of HCl to H_2SO_4 ?

Identify the strong electrolyte.

Calculate the solubility product of Ca(OH)_2 if solubility of it is 3 mol dm^ -3 at 25^ ^ ∘ C .

Which of the following aqueous salt solutions is acidic?

What is the pH of buffer solution containing 10 times higher molar concentration of weak base than the molar concentration of salt of weak base with strong acid at 298 K? (K_b of

Find the pH of 0.02\ M\ HCl .

The solubility product of aluminium hydroxide at 298 K is 4.2 × 10^ -14 . Calculate its solubility in mol/L at same temperature.

Find the p K_b of the weak base BOH, if its K_b is 1 × 10^ -5 ?

Dissociation constant values for H_2CO_3 , CH_3COOH , HCN, and HF are 4.3 × 10^ -7 , 1.8 × 10^ -5 , 4.0 × 10^ -10 and 7.2 × 10^ -4 respectively, at 25^ ^ ∘ C . Identify the

If K_a of weak acid HA is 1 × 10^ -7 , calculate the [H_3O^+] of 0.1\ M solution at equilibrium.

Calculate the pH of the resulting solution obtained by mixing 60\ mL0.1\ M HCl and 40\ mL0.1\ M NaOH.

In the washing of precipitates, the wash liquid should contain a common ion with the precipitate for

The degree of dissociation of a monobasic acid in its 0.1M solution at 300 K is 1.342 × 10^ -2 . Calculate the degree of dissociation of the same acid in its 0.02M solution.

Calculate the percent dissociation of a weak mono-acidic base if its concentration is 0.02 M. [ K_b for weak mono-acidic base = 1.8 × 10^ -5 ]

Identify from following an example of Lewis acid.

In a qualitative analysis Bi^ 3+ is detected by appearance of precipitate of BiO(OH)(s) . Calculate pH when the following equilibrium exists at 298 K : BiO(OH)(s) leftharpoons

At 298 K, a certain buffer solution contains equal concentrations of X^ - and HX , K_b for X^ - is 10^ -10 . What is the pH of this buffer solution ?

The correct order of solubility of the given salts in water at 298 K is Salt K_ sp at 298 K AgBr 5.0×10^ -13 Zn(OH) _2 1.0×10^ -15 Hg _2 Cl _2 1.3×10^ -18

Phenolphthalein is used as an indicator for the titration of sodium hydroxide solution against a standard solution of oxalic acid. The colour change that is observed at an

Phosphoric acid ionizes in three steps with their ionization constant values K_ a_1 , ~K_ a_2 and K_ a_3 , respectively, While K is the overall ionization constant. Which of the

The ratio of solubility of AgCl in 0.1 M KCl solution to the solubility of AgCl in water is: (Given : Solubility product of AgCl=10^ -10 )

Which indicator is used in the titration of sodium hydroxide against oxalic acid and what is the colour change at the end point?

An acidic buffer is prepared by mixing:

For a weak acid HA , the percentage of dissociation is nearly 1 \% at equilibrium. If the concentration of acid is 0.1 ~mol ~L^ -1 , then the correct option for its K_ a at the

Amongst the given options which of the following molecules/ion acts as a Lewis acid?

The pH of the solution containing 50mL each of 0 . 10M sodium acetate and 0 . 01M acetic acid is [Given pK _ a of CH _ 3 COOH = 4 . 57 ]

0.01 M acetic acid solution is 1 \% ionised, then pH of this acetic acid solution is :

The pK _ b of dimethylamine and pK _ a of acetic acid are 3 . 27 and 4 . 77 respectively at T ( K ) . The correct option for the pH of dimethylammonium acetate solution is:

The solubility product for a salt of the type AB is 4 × 10 ^ - 8 . What is the molarity of its saturated solution?

HCl was passed through a solution of CaCl _ 2 , MgCl _ 2 and NaCl . Which of the following compound(s) crystallise(s)?

Find out the solubility of Ni (OH) _ 2 in 0.1MNaOH . Given that the ionic product of Ni (OH) _ 2 is 2 × 10 ^ – 15 .

Which among the following salt solutions is basic in nature?

Assertion : Some salts are sparingly soluble in water at room temperature. Reason : The entropy increases on dissolving the salts.

Which of the following has maximum solubility at low pH ?

If 50 ml of 0.1 HBr is mixed with 50 ml 0.2 M NaOH , find pH of resulting mixture

The pH of 0.01 M NaOH(a q) solution will be

Which of the following cannot act both as Bronsted acid and as Bronsted base?

The molar solubility of CaF_2 (K_ sp =5.3 × 10^ -11 ) in 0.1 M solution of NaF will be

pH of a saturated solution of Ca (OH) _ 2 is 9 . The solubility product ( K _ sp ) of Ca (OH) _ 2 is:

Calculate ionisation constant for pyridinium hydrogen chloride. (Given that H^ + ion concentration is 3.6 × 10^ -4 M and its concentration is 0.02 M .)

When 50 ~mL of 0.1 M NH_3 is mixed with 10 ~mL of 0.1 M HCl then what is the pH of resultant solution? (p K_b=4.75)

Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations. (i) 60mL(M)/(10)HCl + 40mL(M)/(10)NaOH (ii) 55mL(M)/(10)HCl +

The solubility of BaSO _ 4 in water is 2 .42 × 10 ^ - 3 gL ^ - 1 at 298K . The value of its solubility product ( K _ sp ) will be (Given- the molar mass of BaSO _ 4 = 233g mol ^

Calculate the overall complex dissociation equilibrium constant for the [Cu(NH_3)_4]^ 2+ ions, given that stability constant (β_4) for this complex is 2.1 × 10^ 13 .

ZnO is white when cold and yellow when heated. It is due to the development of

K_a for HCN is 5 × 10^ -10 at 25^ ∘ C . For maintaining a constant pH=9 , the volume of 5 M KCN solution required to be added to 10 ~mL of 2 M HCN solution is

When 750 mL of 0.5 M HCl is mixed with 250 mL of 2 M NaOH solution, the value of pH will be

Concentration of the Ag ^ + ions in a saturated solution of Ag _ 2 C _ 2 O _ 4 is 2 .2 × 10 ^ - 4 mol L ^ - 1 . Solubility product of Ag _ 2 C _ 2 O _ 4 is

Assertion : H_2 ~S is stronger acid than PH_3 . Reason : S is more electronegative than P , conjugate base HS^ - is more stable than H_2 P^ - .

K_p for the reaction A leftharpoons B is 4 . If initially only A is present then what will be the partial pressure of B after equilibrium?

100 mL of a solution contains 2 g of acetic acid and 3 g of sodium acetate providing K_a=1.8 × 10^ -5 , then choose the correct option.

Aqueous solution of AlCl_3 is acidic towards litmus while of NaCl is not. The correct reason behind this is

The percentage of pyridine ( C _ 5 H _ 5 N) that forms pyridinium ion ( C _ 5 H _ 5 N ^ + H) in a 0 . 10M aqueous pyridine solution ( K _ b for C _ 5 H _ 5 N = 1 .7 × 10 ^ - 9 ) is

The solubility of AgCl(s) with solubility product 1.6 × 10 ^ - 10 in 0.1MNaCl solution would be

MY and N Y _ 3 , two nearly insoluble salts, have the same K _ sp values of 6.2 × 10 ^ - 13 at room temperature. Which statement would be true in regard to MY and N Y _ 3 ?

The pair of amphoteric hydroxides is

Assertion: Sb_2 ~S_3 is not soluble in yellow ammonium sulphide. Reason : The common ion effect due to S^ 2- ions reduces the solubility of Sb_2 ~S_3 .