# How does Ksp relate to solubility?

Aug 18, 2016

Ksp is the constant of or ratio of the amount of solute to solvent for any compound.

#### Explanation:

K sp is often written in scientific notation like 2.5 x ${10}^{-} 3$

The larger the negative exponent the less soluble the compound is in solution.

The larger the real value of the Ksp the more soluble the compound is in solution 2.5 x ${10}^{-} 3$ > 2.5 x ${10}^{-} 6$

Aug 18, 2016

${K}_{\text{sp}}$ refers to the $\text{solubility product}$. It is another equilibrium expression.

#### Explanation:

For a sparingly soluble binary salt, $M X$, we may write its solubility equilibrium as:

$M X \left(s\right) r i g h t \le f t h a r p \infty n s {M}^{+} + {X}^{-}$

${K}_{\text{sp}} = \left[{M}^{+}\right] \left[{X}^{-}\right]$

Usually ${K}_{\text{sp}}$ assumes standard conditions of temperature and pressure. See here for further treatment. For once I found the appropriate link.