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Answer:
[tex][Ag^+]=1.3x10^{-5}M[/tex]
Explanation:
Hello there!
In this case, according to the dissociation of silver chloride in aqueous solution, we can write:
[tex]AgCl(s)\rightarrow Ag^+(aq)+Cl^-(aq)[/tex]
Whereas the equilibrium expression is:
[tex]Ksp=[Ag^+][Cl^-][/tex]
And the solubility product constant is 1.7 x10⁻¹⁰; thus, by inserting x as the concentration of both silver and chloride ions as they are the same at equilibrium, we obtain:
[tex]1.7x10^{-10}=x^2\\\\x=\sqrt{1.7x10^{-10}} \\x=1.3x10^{-5}M[/tex]
Which is also equal to the concentration silver ions at equilibrium in a saturated solution because we considered the Ksp.
[tex][Ag^+]=1.3x10^{-5}M[/tex]
Best regards!