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The solubility of AgCl is 18 × [tex]10^-^1^0[/tex] in a 0.1M solution of CuCl₂.
The amount of a substance that can dissolve completely in a solvent at a specific temperature is known as its solubility. A saturated solution is one such example.
The maximum number of moles per liter of solution can be dissolved before the solution becomes saturated.
The equilibrium in the saturated solution will be as :
[tex]AgCl[/tex] ⇄ [tex]Ag ^+ + Cl ^-[/tex]
[tex]a[/tex] [tex]a[/tex] [tex]a[/tex]
[tex]CuCl_2[/tex] ⇄ [tex]Cu^2^+ + Cl^-[/tex]
[tex]0.1[/tex] [tex]0.1[/tex] [tex]0.1[/tex]
Ksp = [tex]1.8[/tex] × [tex]10^ -^1^0[/tex]
The solubility product constant: Ksp is the equilibrium constant for the dissolving of an ionic compound in water. Ksp is a function of temperature.
[tex]ksp AgCl = [ Ag ^+ ] [ Cl^-]\\[/tex]
[tex]= a[/tex]×[tex][ a + 0.1][/tex]
[tex]= a^2 + 0.1a[/tex]
[tex]a^2[/tex] is very small, so it is neglected.
ksp AgCl = 0.1a
[tex]1.8[/tex] × [tex]10^ -^1^0[/tex] = 0.1a
a = 18 × [tex]10^-^1^0[/tex]
Therefore, the solubility of AgCl is 18 × [tex]10^-^1^0[/tex].
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