Quantrex Quantrex AcademyJEE · NEET · NDA PYQs with solutions Open app
JEE MainChemistryIonic Equilibrium

A solution contains 0.1 M of A ⁺ ions and 0.2 M of B ²⁺ ions. A precipitating agent containing SO ₄²⁻ ions is added gradually to the solution. It is observed that the salts A ₂ SO ₄ and BSO ₄ begin to precipitate simultaneously. If the solubility product K _ sp of A ₂ SO ₄ is 4.0 10⁻⁸ at the given temperature, what is the solubility product K _ sp of BSO ₄ ?

Options

  1. A8.0 10⁻⁷
  2. B8.0 10⁻⁸
  3. C3.2 10⁻¹²
  4. D4.0 10⁻⁶

Correct answer

A. 8.0 10⁻⁷

Step-by-step solution

For the precipitation of A ₂ SO ₄ , the condition is: [ A ⁺ ]^2 [ SO ₄²⁻ ] = K _ sp ( A ₂ SO ₄) Substituting the given values: (0.1)^2 [ SO ₄²⁻ ] = 4.0 10⁻⁸ 0.01 [ SO ₄²⁻ ] = 4.0 10⁻⁸ [ SO ₄²⁻ ] = 4.0 10⁻⁶ M Since BSO ₄ precipitates simultaneously, it requires the exact same concentration of SO ₄²⁻ ions to initiate precipitation. The condition for BSO ₄ is: [ B ²⁺ ] [ SO ₄²⁻ ] = K _ sp ( BSO ₄) Substituting the values: K _ sp ( BSO ₄) = (0.2) (4.0 10⁻⁶) = 8.0 10⁻⁷ Answer: 8.0 10⁻⁷

Practice Ionic Equilibrium on Quantrex Academy →

More from Ionic Equilibrium

Given is a concentrated solution of a weak electrolyte A_xB_y of concentration 'c' and dissociation constant 'K'. The degree of dissociation is given by : 2026M₃ A₂ is a sparingly soluble salt of molar mass y g mol ⁻¹ and solubility x g L ⁻¹ . The ratio of the molar concentration of the anion ( A³⁻ ) to the solubility product of the salt 2026Arrange the following resultant mixtures in increasing order of their pH values A. 10 mL 0.2 M Ca(OH)₂ + 25 mL 0.1 M HCl B. 10 mL 0.01 M H₂ SO₄ + 10 mL 0.01 M Ca(OH)₂ C. 10 mL 0.1 202620 mL of a solution of acetic acid required 28.4 mL of 0.1 M NaOH for its neutralization. A solution (X) was prepared by mixing 20 mL of the above acetic acid and 14.2 mL of 0.1 M 2026The pH of a solution obtained by mixing 5 mL of 0.1 M NH₄OH solution with 250 mL of 0.1 M NH₄Cl solution is _____ 10⁻² . (Nearest integer) Given: pK_b(NH₄OH) = 4.74 2 = 0.30 3 = 0. 2026The first and second ionization constants of a weak dibasic acid H₂ A are 8.1 10⁻⁸ and 1.0 10⁻¹³ respectively. 0.1 mol of H₂ A was dissolved in 1 L of 0.1 M HCl solution. The conce 2026At 25°C , 20.0 mL of 0.2 M weak monoprotic acid HX is titrated against 0.2 M NaOH. The pH of the solution (a) at the start of the titration (when NaOH has not been added) and (b) w 2026The solubility product constants of Ag₂CrO₄ and AgBr are 32x and 4y respectively at 298 K. The value of ( molarity of Ag₂CrO₄ molarity of AgBr ) can be expressed as : 2026 Full Ionic Equilibrium list All JEE Main PYQs