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Solubility and Solubility Product MCQ - Practice Questions with Answers

Edited By admin | Updated on Sep 25, 2023 25:23 PM | #NEET

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  • Solubility and Solubility Product is considered one the most difficult concept.

  • 33 Questions around this concept.

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QuestionMEDIUM

pH of a saturated solution of  Ca(OH)_2  is 9. The solubility product (K_{sp}) of Ca(OH)_2 is:

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The solubility of BaSO_4 in water is 2.42 \times 10^{-3} gL^{-1} at 298 K. The value of its solubility product (Ksp) will be
(Given molar mass of BaSO_4 = 233 g mol^{-1})

 

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Using the Gibbs energy change, \Delta G^o=+63.3 kJ, for the following reaction,
Ag_2CO_3 (s) \rightarrow 2Ag^+(aq) + CO_3^2^-

The K_s_p of Ag_2CO_3(s) in water at 25^oC is: (R = 8.314 J K^{-1} mol^{-1})

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The pH of a saturated solution of Ba(OH)_2 is 12. The value of the solubility product (K_{SP}) of Ba(OH)_2  is :

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Identify the correct order of solubility in aqueous medium:

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Find out the solubility of Ni(OH)_{2}  in 0.1 M NaOH. Given that the ionic product of Ni(OH)_{2} is 2 \times 10^{-15}.

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The solubility of AgCl (s) with solubility product in 0.1 M NaCl solution would be:

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MY and NY_3 two nearly insoluble salts, have the same K_s_p values of 6.2\times 10^{-13} at room temperature. Which statement would be true in regard of MY and NY_3?

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Identify the correct order of solubility in aqueous medium:

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The K_{sp} \ of \ Ag_{2}CrO_{4}, AgCl, AgBr\ and\ AgI are respectively, 1.1\times 10^{-12}, 1.8\times 10^{-10}, 5.0\times 10^{-13}, 8.3\times 10^{-17}. Which one of the following salts will precipitate last if AgNO_{3} solution is added to the solution containing equal moles of Na_{2}CrO_{4}?

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Concepts Covered - 1

Solubility and Solubility Product

Solubility

It is the weight of solute present in 100 ml of solvent. It is denoted by 's' and is expressed in mol per litre or gm per litre. The number of moles of solute in 1 L of saturated solution is known as molar solubility.

Solubility decreases with the increase in concentration of common ion. It increases with temperature and increases in case the ions formed from the sparingly soluble salt undergo some sort of reaction like complexation.

Example, The solubility of AgCl in water in presence of AgNO3

Solubility increases due to complex ion formation. For example, AgCl has more solubility in ammonia due to complex formation
\mathrm{AgCl + 2NH_3 \rightleftharpoons Ag(NH_3)_2Cl}

Solubility Product: It is the product of the molar concentrations of ions of an electrolyte in a saturated solution at a particular temperature. It is denoted by Ksp or S.

General Representation
\mathrm{A_xB_y} \rightleftharpoons \mathrm{xA}^{+y}+\mathrm{yB}^{-\mathrm{x}}

\mathrm{Ksp =[ A^{+y}]^x \times[ B^{-x}]^y}
 

Relation between Solubility(s) and Solubility Product (Ksp)
\mathrm{A_xB_y} \rightleftharpoons \mathrm{xA}^{+y}+\mathrm{yB}^{-\mathrm{x}}
    s                0             0
    -                xs            ys
\text { Thus, } \mathrm{Ksp = x ^{x} y ^{y}( s )^{ x + y }}


Solubility Product and Precipitation
 

  • If Ksp ≈ Ionic product 
    The solution is saturated and for precipitation, more solute is to be added.
  • If Ionic product > Ksp
    The solution is supersaturated so easily precipitated.
  • If Ionic product < Ksp
    The solution is unsaturated so no precipitation takes place.

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Solubility and Solubility Product

Study other Related Concepts

Solubility and Solubility Product Current Topic

Equilibrium
Law Of Mass Action
Equilibrium Constant
Relation between Kp and Kc
Degree of Dissociation
Le Chatelier's Principles on Equilibrium
Ionic Equilibrium
Bronsted Lowry and Lewis Acid-Base theory
Ionization Of Acids And Bases
Ka and Kb Relationship

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