We’re being asked to calculate the freezing temperature the resultant solution, assuming that the reaction goes to completion.

When calculating the freezing point of a solution, we’re going to use the equation for Freezing Point Depression.

$\overline{){\mathbf{\u2206}}{{\mathbf{T}}}_{{\mathbf{f}}}{\mathbf{=}}{\mathbf{i}}{\mathbf{\xb7}}{{\mathbf{K}}}_{{\mathbf{f}}}{\mathbf{\xb7}}{\mathbf{m}}}$

∆T_{f} = change in freezing point = T_{f pure solvent} –T_{f solution}

K_{f} = freezing point depression constant

i = van' t Hoff factor of the solute = no. of ions

m = molality

We're going to calculate the freezing point of the solution using the following steps:

**Step 1:** Calculate the moles of lithium (Li).**Step 2:** Calculate the moles of LiOH produced.**Step 3:** Calculate the molality of the solution (LiOH).**Step 4:** Calculate the change in temperature (ΔT_{f}).**Step 5: **Calculate the freezing point of the solution.

**Step 1:** Calculate the moles of lithium (Li).

A small cube of lithium (density = 0.535 g/cm^{3}) measuring 1.0 mm on each edge is added to 0.510 L of water. The following reaction occurs:

2 Li(s) + 2 H_{2}O(l) → 2 LiOH(aq) + H_{2}(g)

What is the freezing point of the resultant solution, assuming that the reaction goes to completion?

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