The question is incomplete, the complete question is;
Why was it necessary to make sure that some solid was present in the main solution before taking the samples to measure Ksp? Select the option that best explains why. Choose... A. To make sure no more sodium borate would dissolve in solution. B. To ensure the dissolution process was at equilibrium. C. To make sure the solution was saturated with sodium and borate ions. D. All of the above
Answer:
B. To ensure the dissolution process was at equilibrium.
Explanation:
The solubility product is a term used in chemistry to describe the equilibrium between the dissolved, dissociated and undissolved solute of a relatively low solubility ionic solid.
For an ionic solid MX, the solubility product is given as ;
MX(s) ----> M^n+(aq) + X^n-(aq)
If Ksp indeed scribes an equilibrium process for dissolution, it then implies that some undissolved solute must be present before samples are taken to measure the Ksp of a sample. This ensures equilibrium between dissolved and undissolved solute.
