Calculate the molality of nonvolatile solution if solution freezes at -0.95^ C [ K _ f . for water =1.86 ~K ~kg ~mol ⁻¹ , freezing point of water .=0^ C ]

Step-by-step solution

The freezing point depression is given by T_f = K_f m , where T_f is the freezing point change, K_f is the cryoscopic constant, and m is the molality. For the solution, T_f = 0^ C - (-0.95^ C ) = 0.95 K . Substituting known values, m = 0.95 K 1.86 K kg mol ⁻¹ 0.511 mol kg ⁻¹ . This result does not match any provided option, suggesting a likely error in the problem statement. Assuming the intended freezing point was -0.095^ C , then T_f = 0.095 K , yielding m = 0.095 K 1.86 K kg mol ⁻¹ 0.051 mol kg ⁻¹ , which corres