When dissolved in 1000 g of water, which chemical compound will produce a solution with the greatest freezing point depression?
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To determine which chemical compound will produce a solution with the greatest freezing point depression when dissolved in water, we need to consider the properties of different compounds and their effect on freezing point depression.
The formula for freezing point depression (ΔTf) is given by the equation ΔTf = Kf * m * i, where Kf is the cryoscopic constant, m is the molality of the solute, and i is the van't Hoff factor.
The cryoscopic constant (Kf) is a constant that depends on the solvent being used. For water, the Kf value is 1.86 °C/m.
The molality (m) is the amount of solute dissolved in the solvent, expressed in moles of solute per kilogram of solvent (mol/kg).
The van't Hoff factor (i) takes into account whether the solute dissociates or remains as an undissociated molecule in solution. For compounds that dissociate into ions, such as ionic compounds, i is greater than 1. For compounds that do not dissociate, i is equal to 1.
To determine which compound will produce the greatest freezing point depression, we need to look for a compound that has a high molality (m) and a high van't Hoff factor (i). Additionally, the molality of the compound should be relatively high compared to other compounds considered.
Some compounds that commonly show significant freezing point depression in water are salts, such as sodium chloride (NaCl), calcium chloride (CaCl2), and potassium chloride (KCl). These salts dissociate into ions when dissolved in water, resulting in higher van't Hoff factors (i). Additionally, they have higher molar masses, which means a higher molality (m) for the same weight/volume of solution.
Considering these factors, calcium chloride (CaCl2) is the compound that will produce a solution with the greatest freezing point depression when dissolved in water.