Understanding Solubility
* "Like dissolves like": This principle states that substances with similar polarities are more likely to dissolve in each other.
* Polarity: Polar molecules have uneven distributions of electron density, creating partial positive and negative charges. Nonpolar molecules have a relatively even distribution of electron density.
Analyzing the Compounds
* CBr4 (Carbon Tetrabromide): CBr4 is a nonpolar molecule due to the symmetrical arrangement of the bromine atoms around the central carbon.
* Water (H2O): Water is a highly polar molecule due to the bent shape and the electronegative oxygen atom.
Let's analyze each option:
A. NaCl (Sodium Chloride): Ionic compound, highly polar, will dissolve in water (due to strong ion-dipole interactions). It will not dissolve in CBr4.
B. HCl (Hydrogen Chloride): Polar molecule due to the electronegativity difference between hydrogen and chlorine. It will be slightly soluble in water and even less soluble in CBr4.
C. CH3OH (Methanol): Polar molecule due to the presence of a hydroxyl group (-OH). It will be soluble in water (hydrogen bonding) and slightly soluble in CBr4.
D. CH4 (Methane): Nonpolar molecule. It will be more soluble in CBr4 (due to similar nonpolar interactions) and practically insoluble in water.
E. C2H6 (Ethane): Nonpolar molecule. It will be more soluble in CBr4 (due to similar nonpolar interactions) and practically insoluble in water.
Conclusion
* Most soluble in CBr4: CH4 and C2H6 (due to similar nonpolar character)
* Most soluble in water: NaCl (due to strong ion-dipole interactions)
Important Note: Solubility is a complex phenomenon and can be affected by various factors (temperature, pressure, etc.). The above analysis provides a general understanding of the solubility trends based on polarity.
