Question

Our experimental Ksp for Ca(OH)2 was found to be 2.95 x10^5: when comparing this value to the literature value of 5.02 x 10 ^-6 (CRC Ref. book); Can someone please explain to me some possible experimental or environmental factors for this difference in Ksp?

Answer 1

1.

Temperature is the important factor while conducting this experiment.

Solubility is regulated by temperature, with salts dissolving more readily at higher temperatures. So if room temperature was colder than theoretical, your Ksp will be a larger number (i.e. less soluble) or if it was hotter than theoretical it will be a small number (i.e. more soluble)

2.

Presence of common ions.

Presence of common ions decrease the solubility.

3.

Solvent impurities.

If th solvent has impurities that could solubilize the salts, ksp decreases.