Question #854b9
1 Answer
Explanation:
Notice that the problem provides you with the molar solubility of the salt, i.e. the number of moles that can be dissolved per liter of solution in order to have a saturated solution of
In your case, you know that
You can thus say that the molar solubility of the salt,
#s = "0.0630 mol L"^(-1)#
Now, you know that when
#"AB"_ ((s)) rightleftharpoons "A"_ ((Aq))^(+) + "B"_ ((aq))^(-)#
Notice that every mole of
#["A"] = ["B"]#
Since you already know the molar solubility of the salt at
#["A"] = ["B"] = s#
which means that you have
#["A"] = ["B"] = "0.0630 mol L"^(-1)#
By definition, the solubility product constant,
#K_(sp) = ["A"] * ["B"]#
This means that you have--I won't add the units here
#K_(sp) = 0.0630 * 0.0630 = color(darkgreen)(ul(color(black)(3.97 * 10^(-3))))#
The answer is rounded to three sig figs.