Here's what I got.
Molar solubility is all about the number of moles of a given ionic compound that can be dissolved in one liter of saturated aqueous solution.
In other words, a compound's molar solubility tells you how many moles of said compound can be dissolved in exactly one liter of water in order to make a saturated aqueous solution.
Now, zinc carbonate,
When you dissolve zinc carbonate in water, an equilibrium is established between the undissolved solid and the dissolved ions
#"ZnCO"_ (3(s)) rightleftharpoons "Zn"_ ((aq))^(2+) + "CO"_ (3(aq))^(2-)#
Notice that every mole of zinc carbonate that dissociates produces
The solubility product constant,
#K_(sp) = ["Zn"^(2+)] * ["CO"_3^(2-)]#
The expression of the solubility product constant uses equilibrium concentrations.
If you take
#["Zn"^(2+)] = ["CO"_3^(2-)] = s#
This means that you have
#K_(sp) = s * s = s^2#
Rearrange to solve for
#s = sqrt(K_(sp))#
Plug in your value to find
#1.46 * 10^(-10) = s^2 implies s = sqrt(1.46 * 10^(-10)) = 1.21 * 10^(-5)#
Therefore, you have
#color(darkgreen)(ul(color(black)(s = 1.21 * 10^(-5)"M"))) ->#molar solubility
The answer is rounded to three sig figs.
So, you can say that you can only dissolve