ha. Chs) Which of e following nondissociating) st freezing a c 0.1mCaCl_(2)(aq) 0.1mNaCl(aq) b. 0.1mHF(aq) d 0.1mCH_(3)OH(aq) should have the same freezing point.

The correct answer is:<br /><br />d. $0.1mCH_{3}OH(aq)$<br /><br />Explanation:<br /><br />The freezing point of a solution is determined by the presence of solute particles. In this case, we are looking for the solution that does not dissociate into ions when dissolved in water, as this will result in a lower freezing point compared to solutions that dissociate.<br /><br />a. $0.1mCaCl_{2}(aq)$ - Calcium chloride dissociates into $Ca^{2+}$ and $2Cl^{-}$ ions, which will lower the freezing point.<br /><br />b. $0.1mHF(aq)$ - Hydrofluoric acid is a weak acid and dissociates to some extent, producing $H^{+}$ and $F^{-}$ ions, which will lower the freezing point.<br /><br />c. $0.1mNaCl(aq)$ - Sodium chloride dissociates into $Na^{+}$ and $Cl^{-}$ ions, which will lower the freezing point.<br /><br />d. $0.1mCH_{3}OH(aq)$ - Methanol is a non-dissociating solute and does not produce ions when dissolved in water. Therefore, it will not lower the freezing point as much as the other solutions.<br /><br />Therefore, the solution that should have the same freezing point as the pure solvent is $0.1mCH_{3}OH(aq)$.