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Chapter 1: Problem 15

150 \(\mathrm{mL}\) of saturated \(\mathrm{SrF}_{2}\) solution is present in a 250 \(\mathrm{mL}\) beaker at room temperature. The molar solubility of \(\mathrm{SrF}_{2}\) at 298 \(\mathrm{K}\) is \(1.0 \times 10^{-3} \mathrm{M}\) . If some of the solution evaporates overnight, which of the following will occur? (A) The mass of the solid and the concentration of the ions will stay the same. (B) The mass of the solid and the concentration of the ions will increase. (C) The mass of the solid will decrease, and the concentration of the ions will stay the same. (D) The mass of the solid will increase, and the concentration of the ions will stay the same.

Short Answer

Expert verified
The correct choice is (B) The mass of the solid and the concentration of the ions will increase.

Step by step solution

01

Understanding the Evaporation Process

When some of the solution evaporates, the volume of the solution decreases. However, the amount of the dissolved solute, \( \mathrm{SrF}_2 \), (in moles) remains constant because evaporation only affects the solvent, not the solute. This leads to an effect: the molarity (amount of solute in moles/volume of solution in liter) increases.
02

Determine the Effect on Solid Mass

The mass of the solid \( \mathrm{SrF}_2 \) remains the same. There's nothing in the problem statement that suggests more solid forms or dissolves, there's only evaporation of solvent. Thus, the solid mass is not affected by the evaporation.
03

Determine the Effect on Ion Concentration

The concentration of the ions increases as the solution volume decreases due to evaporation. As the volume of solvent decreases, the number of moles of the solute per liter of solvent increases. This leads to higher concentration in molarity (M) which is defined as moles of solute per liter of solution.

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