Question #32388
1 Answer
For part (b)
Explanation:
I'll show you how to find the molar solubility of silver carboinate,
Silver carbonate is considered insoluble in aqueous solution, which means that it does not dissociate completely into silver cations,
Actually, the fact that it doesn't dissociate completely is an understatement. When silver carbonate is placed in aqueous solution, an equilibrium reaction is established
#"Ag"_2"CO"_text(3(s]) rightleftharpoons 2"Ag"_text((aq])^(+) + "CO"_text(3(aq])^(2-)#
The solubility product constant,
The smaller the value of
To find the molar solubility of silver carbonate, use an ICE table
#"Ag"_2"CO"_text(3(s]) " "rightleftharpoons" " color(red)(2)"Ag"_text((aq])^(+)" " + " " "CO"_text(3(aq])^(2-)#
By definition,
#K_(sp) = ["Ag"^(+)]^color(red)(2) * ["CO"_3^(2-)]#
#K_(sp) = (2s)^2 * s = 4s^2 * s = 4s^3#
This means that
#s = root(3)(K_(sp)/4) = root(3)( (6.2 * 10^(-12))/4) = color(green)(1.2 * 10^(-4)"M")#