That is the maximum. Remember that. The ksp is used to solve for the molar solubility. If the concentration is less, then that amount is dissolved. .01 is greater than .0001. If the molar solubility were 10 M/L and I have 1 M/L then all of it will dissolve and the amount of moles is 1 mole assuming one liter. However, if I have 100M/L. Then, only 10 Moles will dissolve and 90 moles won't. HTH.If you have a 0.0001 M solution of HCl, why do you get 0.0001 mol H+ and 0.0001 mol Cl-?
If you use the Ksp = [H+][Cl-] = 0.0001, you would get [H+] = 0.01 mol.
Why is this not the case?
I think you are confusing Ksp and Ka. You can have a strong base that isn't fully soluble (I think Mg(OH)2 is one such example).Thanks will. So basically with strong acids/bases, it dissociates completely, so you don't need to know the Ksp (just know the molarity), but with weak acids/bases, you only get partial dissociation, so you need to know the Ksp.
So whether or not you use the Ksp value depends on what compound you have, right?
This is absolutely right. Ksp refers to molar solubility when solute is dissolved in solvent. The concept of Ksp is usually applicable to salts. Whenever the ion product is > than its Ksp, the percipitate will form. Mg(OH)2 has a pretty low Ksp value. Meaning if Q>Ksp, the percipitate will form.I think you are confusing Ksp and Ka. You can have a strong base that isn't fully soluble (I think Mg(OH)2 is one such example).