Whatare the molar concentrations of all ions in a 500 mL saturated solution of silver chloride at 25 degrees Celsius?
1 Answer
Explanation:
Your strategy here will be to use the solubility product constant,
You can find the value for the
http://bilbo.chm.uri.edu/CHM112/tables/KspTable.htm
So, you know that
#K_(sp) = 1.8 * 10^(-10)#
Silver chloride,
Use an ICE table to find the molar solubility of silver chloride,
#" ""AgCl"_text((s]) " "rightleftharpoons" " "Ag"_text((aq])^(+) " "+" " "Cl"_text((aq])^(-)#
By definition, the solubility product constant will be equal to
#K_(sp) = ["Ag"^(+)] * ["Cl"^(-)]#
In your case, you will have
#1.8 * 10^(-10) = s * s = s^2#
This will give you
#s = sqrt(1.8 * 10^(-10)) = 1.34 * 10^(-5)#
This means that the concentrations of silver cations and of chloride anons in a saturated solution of silver chloride will be equal to
#["Ag"^(+)] = ["Cl"^(-)] = s = 1.34 * 10^(-5)"mol L"^(-1)#
Therefore, the concentration of both ions in your
#["Ag"^(+)] = ["Cl"^(-)] = color(green)(|bar(ul(color(white)(a/a)1.34 * 10^(-5)"M"color(white)(a/a)|)))#
I'll leave the answer rounded to three sig figs.
Do not get confused by the fact that you're dealing with a
The molar solubility represents concentration, not number of moles of solute. This means that the concentration of both ions in a saturated silver chloride solution will be equal to