For each solute, click the button under the better solvent which the better solvent? CCI CH3(CH2)2CH3 H2O H2O NH4NO3 CH3CH2OH NH4Br
The Correct Answer and Explanation is:
The correct solvent choices based on the “like dissolves like” principle are:
- CH3(CH2)4CH3 dissolves best in CCl4, because both are nonpolar.
- NH4NO3 dissolves best in H2O, as it is an ionic compound and water is a highly polar solvent.
- NH4Br dissolves best in CH3CH2OH, since ethanol is polar and can solubilize ionic compounds.
Explanation
Solubility is governed by intermolecular forces and the nature of the solute and solvent. The fundamental rule is that polar substances dissolve in polar solvents and nonpolar substances dissolve in nonpolar solvents.
- CH3(CH2)4CH3 and CCl4: The solute, CH3(CH2)4CH3, is a nonpolar hydrocarbon. Carbon tetrachloride (CCl4) is also nonpolar due to its symmetric molecular structure. Nonpolar solvents dissolve nonpolar solutes because the primary interaction is weak London dispersion forces, which are sufficient for dissolving hydrocarbons.
- NH4NO3 and H2O: Ammonium nitrate (NH4NO3) is an ionic compound consisting of NH4⁺ and NO3⁻ ions. Water is highly polar and exhibits hydrogen bonding. The water molecules surround and stabilize the ions through ion-dipole interactions, making it the optimal solvent.
- NH4Br and CH3CH2OH: Ammonium bromide (NH4Br) is another ionic compound. Ethanol (CH3CH2OH) is a polar solvent that has a hydroxyl (-OH) group, enabling it to interact with ionic substances via hydrogen bonding. Though water is more polar than ethanol, ethanol can still effectively dissolve NH4Br due to its ability to form ion-dipole interactions.
Understanding solubility principles is essential in fields such as chemistry, biochemistry, and pharmaceuticals, where solvent selection impacts reactions, separations, and formulations. The correct solvent choice ensures efficient dissolution and optimal chemical processes.
