What is the solubility of a salt? Explain the classification of salts based on solubility.
(N/A) The solubility of a salt is defined as the number of moles of solute that can be dissolved in $1 \ L$ of solvent at a specific temperature.
Classification of salts based on solubility:
$(i)$ Soluble salts:
- Solubility is greater than $0.1 \ M$.
- These salts exist in the form of ions in solution (complete ionization).
- Examples: $NaCl, CaCl_2, CaF_2$.
$(ii)$ Less soluble salts:
- Solubility is between $0.01 \ M$ and $0.1 \ M$.
- These salts exhibit ionic equilibrium in solution.
- Examples: $Ca(OH)_2, MgSO_4$.
$(iii)$ Sparingly soluble salts:
- Solubility is less than $0.01 \ M$.
- These salts are very slightly soluble and form insoluble precipitates in solution.
- Examples: $AgCl, Mg(OH)_2, BaSO_4$.
The solubility of salts varies with temperature.
Classification of salts based on solubility:
$(i)$ Soluble salts:
- Solubility is greater than $0.1 \ M$.
- These salts exist in the form of ions in solution (complete ionization).
- Examples: $NaCl, CaCl_2, CaF_2$.
$(ii)$ Less soluble salts:
- Solubility is between $0.01 \ M$ and $0.1 \ M$.
- These salts exhibit ionic equilibrium in solution.
- Examples: $Ca(OH)_2, MgSO_4$.
$(iii)$ Sparingly soluble salts:
- Solubility is less than $0.01 \ M$.
- These salts are very slightly soluble and form insoluble precipitates in solution.
- Examples: $AgCl, Mg(OH)_2, BaSO_4$.
The solubility of salts varies with temperature.
Explore More
Similar Questions
$A$ precipitate of calcium oxalate will not dissolve in
Medium
View SolutionWhat is the minimum concentration of $SO_4^{2-}$ required to precipitate $BaSO_4$ in a solution containing $1.0 \times 10^{-4} \ M \ Ba^{2+}$ ($K_{sp}$ for $BaSO_4$ is $4 \times 10^{-10}$)?
Medium
View SolutionThe solubility product of $AgCl$ is $1.8 \times 10^{-10}$. Mixing equal volumes of which of the following solutions will result in the precipitation of $AgCl$?
Difficult
View SolutionIn a saturated solution of the sparingly soluble strong electrolyte $AgIO_3$ (molecular mass $= 283$),the equilibrium which sets in is $AgIO_{3(s)} \rightleftharpoons Ag^+_{(aq)} + IO^-_{3(aq)}$. If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 \times 10^{-8}$,what is the mass of $AgIO_3$ contained in $100 \ mL$ of its saturated solution?
MediumAIEEE 2007
View SolutionWhich of the following has the maximum solubility? (Given $K_{sp}$ values)
Easy
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo