JEE Main PYQs — Ionic Equilibrium

10 mL of 2 M NaOH solution is added to 20 mL of 1 M HCl solution kept in a beaker. Now, 10 mL of this mixture is poured into a volumetric flask of 100 mL containing 2 moles of HCl and made the volume…

If equal volumes of AB2 and XY (both are salts) aqueous solutions are mixed, which of the following combination will give a precipitate of AY2 at 300 K? (Given Ksp for AY2 = 5.2 10-7)

A weak acid HA has degree of dissociation x. Which option gives the correct expression of pH - pKa?

An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would (Given 2 = 0.30):

Arrange the following in increasing order of solubility product: {Ca(OH)}_2,\;{AgBr},\;{PbS},\;{HgS}

Identify the inorganic sulphides that are yellow in colour: (A) (NH4)2S (B) PbS (C) CuS (D) As2S3 (E) As2S5 (a) (A) and (C) only (b) (A), (D) and (E) only (c) (A) and (B) only (d) (D) and (E) only

Ksp for Cr(OH)3 is 1.6 10-30. What is the molar solubility of this salt in water? (a) [4]1.6 10-3027 (b) 1.8 10-3027 (c) [5]1.8 10-30 (d) [4]1.6 10-30

HA(aq) H+(aq) + A-(aq) The freezing point depression of a 0.1 m aqueous solution of a monobasic weak acid HA is 0.20°C. The dissociation constant for the acid is Given: Kf(H2O) = 1.8 kg mol-1,…

Given below are two statements: Statement (I): Aqueous solution of ammonium carbonate is basic. Statement (II): Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on Ka…

Which of the following is the strongest Bronsted base?

For a sparingly soluble salt AB2, the equilibrium concentrations of A2+ ions and B- ions are 1.2 10-4 M and 0.24 10-3 M, respectively. The solubility product of AB2 is:

Given below are two statements: Statement I: On passing HCl gas through a saturated solution of BaCl2, at room temperature white turbidity appears. Statement II: When HCl gas is passed through a…

Solubility of calcium phosphate (molecular mass M) in water is W g per 100 mL at 25 °C. Its solubility product at 25 °C will be approximately:

Given below are two statements: Statement (I): A buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities. Statement (II): Blood is a naturally occurring…

Incorrect statement for the use of indicator in acid-base titration is:

Which of the following statement(s) is/are correct? (A) The pH of 1 10-8 M HCl solution is 8. (B) The conjugate base of H2PO4- is HPO42-. (C) Kw increases with increase in temperature. (D) When a…

Given below are two statements: Statement I: Methyl orange is a weak acid. Statement II: The benzenoid form of methyl orange is more intense/deeply coloured than the quinonoid form. Choose the most…

When the hydrogen ion concentration [H+] changes by a factor of 1000, the value of pH of the solution

In base vs. acid titration, at the end point methyl orange is present as

Assertion: The amphoteric behaviour of water is explained by Lewis acid-base theory. Reason: Water acts as acid with NH3 and base with H2S. Choose the correct option:

The Ksp for bismuth sulphide (Bi2S3) is 1.08 10-73. The solubility of Bi2S3 in mol\ L-1 at 298 K is

200 mL of 0.01 M HCl is mixed with 400 mL of 0.01 M H2SO4. The pH of the mixture is

Ka1, Ka2 and Ka3 are the respective ionization constants for the following reactions: (a) H2C2O4 H+ + HC2O4- (b) HC2O4- H+ + C2O42- (c) H2C2O4 2H+ + C2O42- The relationship between Ka1, Ka2 and Ka3…

20 mL of 0.1 M NH4OH is mixed with 40 mL of 0.05 M HCl. The pH of the mixture is nearest to: (Kb(NH4OH) = 1 10-5,\ 2 = 0.30,\ 3 = 0.48,\ 5 = 0.69,\ 7 = 0. 84,\ 11 = 1. 04)

The plot of pH-metric titration of weak base NH4OH vs strong acid HCl looks like which graph?

The solubility of AgCl will be maximum in which of the following?

A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio [CH3CH2COO-][CH3CH2COOH] required to make the buffer is: [Ka(CH3CH2COOH) = 1.3 10-5]

Class XII students were asked to prepare one litre of buffer solution of pH 8.26 by their chemistry teacher. The amount of ammonium chloride to be dissolved by the student in 0.2 M ammonia solution…

Which of the following compound CANNOT act as a Lewis base?

The solubility of Ca(OH)2 in water is: [Ksp of Ca(OH)2 = 5.5 10-6]

Given below are two statements: Statement I: In the titration between strong acid and weak base, methyl orange is suitable as an indicator. Statement II: For titration of acetic acid with NaOH,…

The solubility of AgCN in a buffer solution of pH = 3 is x. The value of x is: [Ksp(AgCN) = 2.2 10-16;\ Ka(HCN) = 6.2 10-10]

A solution is 0.1 M in Cl- and 0.001 M in CrO42-. Solid AgNO3 is gradually added to it. [Ksp(AgCl) = 1.7 10-10\ M2;\ Ksp(Ag2CrO4) = 1.9 10-12\ M3] Select the correct statement:

An acidic buffer is obtained on mixing:

For the following Assertion and Reason, the correct option is: Assertion: The pH of water increases with increase in temperature. Reason: The dissociation of water into H+ and OH- is an exothermic…

Arrange the following solutions in the decreasing order of pOH: (A) 0.01 M HCl (B) 0.01 M NaOH (C) 0.01 M CH3COONa (D) 0.01 M NaCl

The stoichiometry and solubility product of a salt with the solubility curve given below (solubility = 10-3 M at 298 K) is, respectively:

The Ksp for the following dissociation is 1.6 10-5: PbCl2(s) Pb2+(aq) + 2Cl-(aq) Which of the following choices is correct for a mixture of 300 mL 0.134 M Pb(NO3)2 and 100 mL 0.4 M NaCl?

The solubility product of Cr(OH)3 at 298 K is 6.0 10-31. The concentration of hydroxide ions in a saturated solution of Cr(OH)3 will be

The amphoteric hydroxide is:

If solubility product of Zr3(PO4)4 is denoted by Ksp and its molar solubility is denoted by S, then which of the following relations between S and Ksp is correct?

Consider the following statements: (a) The pH of a mixture containing 400 mL of 0.1 M H2SO4 and 400 mL of 0.1 M NaOH will be approximately 1.3. (b) Ionic product of water is temperature dependent.…

In an acid-base titration, 0.1 M HCl solution was added to the NaOH solution of unknown strength. Which of the following correctly shows the change of pH of the titration mixture in this experiment?

20 mL of 0.1 M H2SO4 solution is added to 30 mL of 0.2 M NH4OH solution. The pH of the resultant mixture is: [pKb\ of\ NH4OH = 4.7]

The pH of a 0.02 M NH4Cl solution will be: [Kb(NH4OH) = 10-5,\ 2 = 0.301]

What is the molar solubility of Al(OH)3 in 0.2 M NaOH solution? [Ksp(Al(OH)3) = 2.4 10-24]

A mixture of 100 mmol of Ca(OH)2 and 2 g of sodium sulphate was dissolved in water and the volume was made up to 100 mL. What is the mass of calcium sulphate formed and the concentration of OH- in…

If Ksp of Ag2CO3 is 8 10-12, the molar solubility of Ag2CO3 in 0.1 M AgNO3 is:

The molar solubility of Cd(OH)2 is 1.84 10-5 M in water. The expected solubility of Cd(OH)2 in a buffer solution of pH = 12 is: