To determine the solubility of solid potassium chloride (KCl) in different solvents, we must examine the nature of KCl and the solvents in question.
Potassium chloride (KCl) is an ionic compound. Ionic compounds generally dissolve well in polar solvents due to the positive and negative ions' attraction to the partial charges in polar molecules.
Let's analyze each solvent:
1. [tex]$C_3H_8$[/tex] (Propane):
- Propane is a non-polar molecule because it consists solely of hydrogen and carbon atoms with no significant electronegativity difference.
- Non-polar solvents do not dissolve ionic compounds well.
2. [tex]$CH_3CH_2CH_2CH_2CH_3$[/tex] (Pentane):
- Pentane is also a non-polar molecule, similar to propane, composed of carbon and hydrogen atoms.
- It lacks polarity and therefore does not dissolve ionic compounds like KCl effectively.
3. [tex]$H_2O$[/tex] (Water):
- Water is a highly polar solvent. Its molecules have a significant electronegativity difference between the hydrogen and oxygen atoms, leading to a dipole moment.
- The polarity of water makes it excellent for dissolving ionic compounds such as KCl.
4. [tex]$CH_3CH_2CH_3OH$[/tex] (Propanol):
- Propanol has a polar hydroxyl ([tex]$-OH$[/tex]) group, which gives it some polarity.
- While more polar than hydrocarbons like propane and pentane, it is less polar than water.
- It can dissolve ionic compounds to some degree but not as effectively as water.
Given these analyses, the best solvent for dissolving KCl is the one that is most polar: [tex]$H_2O$[/tex] (Water).
Therefore, solid potassium chloride (KCl) is most likely to be soluble in:
[tex]\[ \boxed{H_2O} \][/tex]
