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. What is the freezing point of a solution of 0.5 mol of LiBr in 500 mL of water (Kf 1.86 and Acirc and degCm)?
To find the freezing point of the solution, we first calculate the molality (m) of the LiBr solution. Since 0.5 mol of LiBr is dissolved in 0.5 kg of water (500 mL of water), the molality is 1.0 m. Using the formula for freezing point depression, ΔTf = Kf * m, where Kf = 1.86 °C/m, we get ΔTf = 1.86 °C/m * 1.0 m = 1.86 °C. Thus, the freezing point of the solution is 0 °C - 1.86 °C = -1.86 °C.
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What information is most useful to determine the solution that has a lower freezing point?
To determine which solution has a lower freezing point, you need the concentrations of solute in each solution and their respective properties (molal freezing point depression constants). The solution with the higher concentration of solute and lower molal freezing point depression constant will have the lower freezing point.
What is the molality of a solution of water and KCl if the freezing point of the solution is and ndash3 and degC (Kf 1.86 and degCm molar mass of water 18 g)?
To find the molality of the KCl solution, we can use the freezing point depression formula: ΔTf = Kf * m * i, where ΔTf is the change in freezing point, Kf is the cryoscopic constant (1.86 °C kg/mol for water), m is the molality, and i is the van 't Hoff factor (which is 2 for KCl, as it dissociates into K⁺ and Cl⁻). The change in freezing point is 0 - (-3) = 3 °C. Rearranging the formula gives us m = ΔTf / (Kf * i), so m = 3 / (1.86 * 2) ≈ 0.806 mol/kg. Therefore, the molality of the KCl solution is approximately 0.806 mol/kg.
Why is the curve for the freezing of a solution different in slope from the freezing of the solvent?
The curve for the freezing of a solution is different from that of the pure solvent because the presence of solute particles lowers the freezing point of the solution. This phenomenon is known as freezing point depression. The slope of the curve for the solution is less steep than that of the solvent due to this depression effect.
What effect does adding solute have on the freezing point of a solution?
the temperature at which the solution freezes is lowered.
What is the molality of a solution of water and KCl if the freezing point of the solution is and ndash3 and degC (Kf 1.86 and degCm molar mass of water 18 g).?
To find the molality of the KCl solution, we can use the freezing point depression formula: (\Delta T_f = K_f \cdot m \cdot i), where (i) is the van 't Hoff factor (which is 2 for KCl). The freezing point depression (\Delta T_f) is 3°C (from 0°C to -3°C). Using (K_f = 1.86 , \text{°C kg/mol}), we can rearrange the formula to find molality (m): [ m = \frac{\Delta T_f}{K_f \cdot i} = \frac{3}{1.86 \cdot 2} \approx 0.805 , \text{mol/kg} ] Thus, the molality of the KCl solution is approximately 0.805 mol/kg.
What is the freezing point of the solution?
The freezing point of a solution is the temperature at which the liquid in the solution solidifies or freezes.
What is the process for using a salt water freezing point calculator to determine the freezing point of a solution?
To determine the freezing point of a solution using a salt water freezing point calculator, you need to input the concentration of salt in the solution and the calculator will provide you with the freezing point of the solution.
Will a 0.5 M solution have a higher freezing point than a 0.75 M solution of the same substance?
No, the 0.75 M solution will have a higher freezing point. The freezing point depression is directly proportional to the molality of the solution, so a higher concentration solution will have a greater effect on lowering the freezing point.
What is the freezing point of a solution that contains 0.550 moles of Nal in 615 g of water?
The freezing point depression equation is used to calculate the freezing point of a solution. Given the molality of the NaI solution and the molecular weight of water, the freezing point of the solution can be determined.
When a solute is added to solvent the freezing point of the solution is?
The freezing point is lowered.
What is the freezing point of a solution containing 2.50g of benzene in 120g of chloroform?
Since benzene is the solute and chloroform is the solvent, this is a non-electrolyte solution. The freezing point depression equation is ΔTf = Kf * m, where ΔTf is the freezing point depression, Kf is the freezing point depression constant for chloroform, and m is the molality of the solution. From this, you can calculate the freezing point of the solution.
What information is most useful to determine the solution that has a lower freezing point?
To determine which solution has a lower freezing point, you need the concentrations of solute in each solution and their respective properties (molal freezing point depression constants). The solution with the higher concentration of solute and lower molal freezing point depression constant will have the lower freezing point.
21.6 g NiSO4 in 1.00 102g Hu2082O what is the freezing point of this solution?
To determine the freezing point of the solution, you need to calculate the molality of the NiSO4 in the H2O solution. Once you have the molality, you can then use the formula for freezing point depression to find the freezing point. This formula is ΔTf = Kf * m, where ΔTf is the freezing point depression, Kf is the freezing point depression constant (for water it is 1.86 °C kg/mol), and m is the molality of the solution. Finally, add the freezing point depression to the normal freezing point of water (0°C) to find the freezing point of the solution.
What is the significance of the freezing point depression constant in determining the freezing point of a solution?
The freezing point depression constant helps determine how much the freezing point of a solution will decrease compared to the pure solvent. This is important because it allows us to calculate the exact freezing point of a solution, which is useful in various scientific and industrial applications.
What is the molality of a solution of water and KCl if the freezing point of the solution is and ndash3 and degC (Kf 1.86 and degCm molar mass of water 18 g)?
To find the molality of the KCl solution, we can use the freezing point depression formula: ΔTf = Kf * m * i, where ΔTf is the change in freezing point, Kf is the cryoscopic constant (1.86 °C kg/mol for water), m is the molality, and i is the van 't Hoff factor (which is 2 for KCl, as it dissociates into K⁺ and Cl⁻). The change in freezing point is 0 - (-3) = 3 °C. Rearranging the formula gives us m = ΔTf / (Kf * i), so m = 3 / (1.86 * 2) ≈ 0.806 mol/kg. Therefore, the molality of the KCl solution is approximately 0.806 mol/kg.
Will NaCl's affect the freezing point of a solution make the freezing point increase?
No, adding NaCl to a solution will actually lower the freezing point of the solution. This is because the presence of dissolved ions from the salt disrupts the formation of ice crystals, causing the freezing point to decrease.
How can one calculate freezing point depression in a solution?
To calculate freezing point depression in a solution, you can use the formula: Tf i Kf m. Tf represents the freezing point depression, i is the van't Hoff factor, Kf is the cryoscopic constant, and m is the molality of the solution. By plugging in these values, you can determine the freezing point depression of the solution.
