Question

Write the balanced equation for the equilibrium reaction for the dissociation ofsilver chloride in water, and write the K expression for this reaction. Then create an ICE chart. Since we know the equilibrium concentration of the silver ion, we can solve for Ksp.Does it agree with the literature value

Answer 1

Answer:

See explanation

Explanation:

Hello there!

In this case, since the the concentrations are not given, and not even the Ksp, we can solve this problem by setting up the chemical equation, the equilibrium constant expression and the ICE table only:

$AgCl(s)\rightleftharpoons Ag^+(aq)+Cl^-(aq)$

Next, the equilibrium expression according to the produced aqueous species as the solid silver chloride is not involved in there:

$Ksp=[Ag^+][Cl^-]$

And therefore, the ICE table, in which x stands for the molar solubility of the silver chloride:

       $\ \ \ \ \ \ \ \ \ \ \ \ \ \ AgCl(s)\rightleftharpoons Ag^+(aq)+Cl^-(aq)$

I          -                   0             0

C        -                   +x           +x

E        -                    x             x

Which leads to the following modified equilibrium expression:

$Ksp=x^2$

Unfortunately, values were not given, and they cannot be arbitrarily assigned or assumed.

Regards!