a) KCl in H2O: High solubility. KCl is an ionic compound that dissociates in water, forming ions that are able to interact with the polar water molecules, resulting in a high solubility.
KCl in CH3OH: Low solubility. CH3OH is a polar solvent but it has weaker polarity and lower dielectric constant than H2O, thus it cannot effectively solvate the ionic K+ and Cl- ions, resulting in a low solubility.
b) HF in H2O: High solubility. HF is a polar molecule that can form hydrogen bonds with water, resulting in a strong solvation of the HF molecules, and hence high solubility.
c) NH4Cl in C5H12: Low solubility. C5H12 (pentane) is a nonpolar solvent and is unable to solvate the ionic NH4+ and Cl- ions effectively, resulting in a low solubility.
d) H2O in CH3OH: High solubility. Both H2O and CH3OH are polar solvents that can form hydrogen bonds with each other, resulting in high solubility.
e) NH4Cl in CCl4: Low solubility. CCl4 is a nonpolar solvent and cannot form strong electrostatic interactions with the ionic NH4+ and Cl- ions, resulting in low solubility.
f) CCl4 in H2O: Low solubility. CCl4 is a nonpolar solvent and incompatible with the polar H2O solvent, resulting in low solubility.
20. Consider the following solutions. In each case, predict whether the solubility of the
solute should be high or low. Justify your answer.
a KCl in H2
O d H2
O in CH3
OH
b HF in H2
O e NH4
Cl in C5
H12
c KCl in CCl4 f CCl4
in H2
O�
1 answer