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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.
34 Questions around this concept.

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H₂COH • CH₂OH on heating with periodic acid gives:

2 HCOOH

2 CO₂

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