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SOLUTION:

Step 1: List the given values.

[tex]\begin{aligned} & mass_{\text{solute}} = \text{34.2 g} \\ & MM_{\text{solute}} = \text{98.08 g/mol} \\ & mass_{\text{solvent}} = \text{173 g = 0.173 kg} \end{aligned}[/tex]

Step 2: Calculate the number of moles of solute.

[tex]\begin{aligned} n_{\text{solute}} & = \frac{mass_{\text{solute}}}{MM_{\text{solute}}} \\ & = \frac{\text{34.2 g}}{\text{98.08 g/mol}} \\ & = \text{0.34869 mol} \end{aligned}[/tex]

Step 3: Calculate the molality of solution.

[tex]\begin{aligned} m & = \frac{n_{\text{solute}}}{mass_{\text{solvent}}} \\ & = \frac{\text{0.34869 mol}}{\text{0.173 kg}} \\ & = \text{2.02 mol/kg} \\ & = \boxed{2.02 \: m} \end{aligned}[/tex]

Hence, the molality of the solution is 2.02 m.

[tex]\\[/tex]

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