Question #75478
1 Answer
Explanation:
The problem essentially wants you to determine the molar solubility of silver chloride, i.e. the maximum number of moles of silver chloride that can be dissolved in
So, you know that silver chloride is insoluble in water. This tells you that when you dissolve this salt in water, most of it will remain undissociated.
The equilibrium that is established between the undissolved salt and the dissolved ions looks like this
#"AgCl"_ ((s)) rightleftharpoons "Ag"_ ((aq))^(+) + "Cl"_ ((aq))^(-)#
The solubility product constant,
#K_(sp) = ["Ag"^(+)] * ["Cl"^(-)]#
Now, notice that when
So you can say that, at equilibrium, the solution has
#["Ag"^(+)] = ["Cl"^(-)]#
If you take
#K_(sp) = s * s#
#K_(sp) = s^2#
Rearrange to solve for
#s = sqrt(K_(sp))#
Plug in your value to find
#K_(sp) = sqrt(1.8 * 10^(-10)) = 1.3 * 10^(-5)#
Since this number represents the number of moles of silver chloride that can be dissolved in
#color(darkgreen)(ul(color(black)("no. of moles AgCl" = 1.3 * 10^(-5)color(white)(.)"moles")))#