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lozanna [386]
3 years ago
9

Calculate the boiling point of a 2.00 molal solution of magnesium perchlorate, mg(clo4)2, in water.

Chemistry
1 answer:
vova2212 [387]3 years ago
5 0

Answer:

103.06°C.

Explanation:

  • To solve this problem, we can use the relation:

<em>ΔTb = i.Kb.m,</em>

Where, i is the van 't Hoff factor.

Kb is the molal boiling point  elevation constant of water (Kb = 0.51°C/m).

m is the molality of the solution (m = 2.0 m).

  • We need to define and find the van 't Hoff factor (i):

<em>van 't Hoff factor</em> is the ratio between the actual concentration of particles produced when the substance is dissolved and the concentration of a substance as calculated from its mass.

  • Mg(ClO₄)₂ is dissociated according to the equation:

<em>Mg(ClO₄)₂ → Mg²⁺ + 2ClO₄⁻,</em>

1 mol of Mg(ClO₄)₂ produces 3 mol of ions (1 mol Mg²⁺ and 2 mol ClO₄⁻).

∴ i = 3/1 = 3.

∴ ΔTb = i.Kb.m = (3)(0.51 °C/m)(2.0 m) = 3.06 °C.

∵  ΔTb = the boiling point in presence of solute (Mg(ClO₄)₂) - the boiling point of pure water.

The boiling point of pure water = 100.0°C.

<em>∴ The boiling point in presence of solute (Mg(ClO₄)₂) = ΔTb + the boiling point of pure water =</em> 3.06 °C + 100.0°C = <em>103.06°C.</em>

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