Answer:
Ksp = [tex]2.57X10^{-9}[/tex]
Explanation:
Molar solubility of barium carbonate will be obtained by dividing the given solubility (in g/L) with molar mass of barium carbonate
molar solubility = [tex]\frac{solubility}{molarmass}=\frac{0.01}{197.3}=5.068X10^{-5}M[/tex]
The barium carbonate will undergo dissociation as:
[tex]BaCO_{3}------>Ba^{+2}+CO_{3}^{-2}[/tex]
Ksp of barium carbonate will be
Ksp = [tex][Ba^{+2}][CO_{3}^{-2}][/tex]
If solubility of barium carbonate is "s"
The concentration of each ion will be "s"
Hence the expression becomes
Ksp = s²
where
s = molar solubility = 5.068 X10⁻⁵
Ksp = [tex]5.068X10^{-5}X5.068X10^{-5}=2.57X10^{-9}[/tex]
