Consider a 1.00 m magnesium nitrate, Mg(NO3)2, aqueoussolution.

a. Determine the molality (in m) of all solutes in the solution.Assume that magnesium nitrate completely ionizes when dissolved inwater. All solutes means all cations and anions. The molality thatyou determine here is the value for msolute of (Equation 3)>>> CaCl2(aq) ? Ca2+(aq) + 2 Cl?(aq) . 3 × 1.0 m =3.0 m Show your work. You must explain your answer instead of onlywriting calculations.

b. Determine the magnitude of the freezing point depression (?T)of the solution. Given that the molal freezing pointdepression constant, Kf, for water is 1.86 °C?kg/mol. Show yourwork. (Hint: Remember that m = mol/kg when m represents themolality.)

c. Determine the freezing point of the solution. The freezingpoint of water is 0°C exactly. Show your work.

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a To determine the molality of all solutes in the magnesium nitrate solution we first need to calcul... View the full answer