QQuestionChemistry
QuestionChemistry
Assuming equal concentrations and complete dissociation, arrange these aqueous solutions by their freezing points.
# Highest freezing point
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| K₂SO₄ | Li₃PO₄ | NaNO₃ | | | | | | | | | | | | | |
12 months agoReport content
Answer
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Step 1:: Understand the problem
The problem asks us to arrange aqueous solutions by their freezing points, assuming equal concentrations and complete dissociation. The solutions given are K₂SO₄, Li₃PO₄, and NaNO₃.
Step 2:: Know the concept
When an electrolyte (like the salts given) is added to water, it dissociates into ions. This increases the number of particles in the solution, which lowers the freezing point. The freezing point depression (ΔTf) is calculated using the formula ΔTf = Kf · m, where Kf is the cryoscopic constant for water (1.86 °C·kg/mol) and m is the molality of the solution. Since the concentrations are equal, the molality will be the same for all solutions, so the relative freezing point depression will depend only on the Kf values of the salts.
Step 3:: Find the Kf values
To find the Kf values, we need to look up the relevant data. The Kf values for K₂SO₄, Li₃PO₄, and NaNO₃ are approximately 3.93, 7.6, and 4.56 °C·kg/mol, respectively.
Step 4:: Compare the Kf values
Now, we can compare the Kf values to determine the relative freezing points of the solutions: - K₂SO₄: 3.93 °C·kg/mol - Li₃PO₄: 7.6 °C·kg/mol - NaNO₃: 4.56 °C·kg/mol
Step 5:: Arrange the solutions by freezing points
Since the Kf values are directly proportional to the freezing point depression, we can arrange the solutions from highest to lowest freezing point as follows:
Final Answer
1. Li₃PO₄ 2. NaNO₃ 3. K₂SO₄ The freezing point decreases as the Kf value increases, so Li₃PO₄ has the highest freezing point, followed by NaNO₃ and K₂SO₄.
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