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How does freezing point get calculated if boiling point of an aqueous solution is given?
Wiki User
∙ 12y ago
F.p.'s and B.p.'s are independent (intensive) properties, you can NOT calculate them.
Wiki User
∙ 12y ago
You can calculate the freezing point of an aqueous solution using the equation for colligative properties: ΔTf = i * Kf * m, where ΔTf is the freezing point depression, i is the van 't Hoff factor, Kf is the cryoscopic constant of the solvent, and m is the molality of the solution. By rearranging the equation, you can solve for the freezing point.
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How do you separate KNO3 from aqueous sol of KNO3?
You can separate KNO3 from its aqueous solution by a process called evaporation. Simply heat the solution to evaporate the water, leaving behind solid KNO3. This method exploits the fact that KNO3 has a much higher boiling point compared to water.
What lowers the freezing point and raises the boiling point?
Adding solutes, such as salt or sugar, to a solvent can lower the freezing point and raise the boiling point. This phenomenon is known as freezing point depression and boiling point elevation, respectively. The presence of solutes disrupts the normal crystal structure in the solvent, requiring lower temperatures to freeze and higher temperatures to boil.
Calculate the boiling point elevation of an aqueous solution of 0.14 m glucose?
The boiling point elevation of a solution can be calculated using the equation ΔTb = i * Kb * m, where i is the van't Hoff factor (1 for glucose), Kb is the ebullioscopic constant for water (0.512 °C/m), and m is the molality of the solution (0.14 m). Plugging in these values, we get ΔTb = 1 * 0.512 * 0.14 = 0.07168 °C. So, the boiling point elevation of the solution is 0.07168 °C.
The physical properties of a solution that differ from those of its solute and solvent include freezing point boiling point and what?
The physical properties of a solution that differ from those of its solute and solvent include boiling point elevation, freezing point depression, osmotic pressure, and vapor pressure changes.
What are freezing and boiling point of 0.1 molar solution of CaCl2 in water?
The influence is extremely low - apprpox. 0,05 0C.
What is the freezing point of an aqueous solution if the boiling point of an aqueous solution is 101.34 degree Celsius?
The freezing point of an aqueous solution will be lower than 0°C (32°F) if the boiling point is elevated above 100°C. The freezing point depression is a colligative property dependent on the concentration of solute particles in the solution. To determine the specific freezing point, more information on the solute and its concentration is required.
Compared to the pure water an aqueous solution of calcium chloride has a?
Higher boiling point and a lower freezing point. These are called colligative properties. When a solute is put into solution with the solvent, there is a change in the vapor pressure, osmotic pressure, elevation of the boiling point, and depression of the freezing point.
What is the boiling point of an aqueous solution that has a vapor pressure of 18.5 at 25 degrees Celsius?
The boiling point of an aqueous solution can be calculated using the formula: ΔT = iKbm, where ΔT is the boiling point elevation, i is the van't Hoff factor, Kb is the ebullioscopic constant, and m is the molality of the solution. Given the vapor pressure of 18.5 mmHg, you can determine the molality of the solution and then calculate the boiling point elevation.
What are some things that are true about boiling points?
The boiling point of 2 m KF in water is 102.4ºC. The boiling point of a 0.5 m aqueous solution of LiOH is the same as the boiling point of a 0.5 m aqueous solution of LiCl.
Explain why the vapor pressure boiling point and freezing point of an aqueous solution if a nonvolatile solute are not the same as those of the pure solvent?
The presence of a nonvolatile solute in an aqueous solution lowers the vapor pressure of the solution, raising its boiling point and lowering its freezing point compared to the pure solvent. This occurs due to the solute molecules occupying space at the surface of the solution, reducing the number of solvent molecules escaping into the vapor phase. As a result, a higher temperature is needed to reach the same vapor pressure as the pure solvent for boiling, and a lower temperature is needed for the solution to freeze.
Is the boiling point of a 0.5 m aqueous solution of KOH higher than the boiling point of a .5m aqueous solution of KCL?
Yes, the boiling point of a 0.5 m aqueous solution of KOH would be higher than the boiling point of a 0.5 m aqueous solution of KCl. This is because KOH is a strong electrolyte that dissociates into more ions in solution compared to KCl, leading to a greater increase in boiling point due to the colligative properties of the solution.
What is the boiling point of concentrated aqueous solution of sodium chloride?
The boiling point of a concentrated aqueous solution of sodium chloride is higher than that of pure water. This is due to the presence of the solute, which raises the boiling point of the solution through a process called boiling point elevation. The exact boiling point will depend on the concentration of the sodium chloride in the solution.
What lowers the freezing point and raises the boiling point?
Adding solutes, such as salt or sugar, to a solvent can lower the freezing point and raise the boiling point. This phenomenon is known as freezing point depression and boiling point elevation, respectively. The presence of solutes disrupts the normal crystal structure in the solvent, requiring lower temperatures to freeze and higher temperatures to boil.
What occurs when NaCl is added to water?
The boiling point of the solution increases, and the freezing point of the solution decreases.
What does ethylene glycol do to the solution?
Raises the boiling point and lowers the freezing point.
How do you separate KNO3 from aqueous sol of KNO3?
You can separate KNO3 from its aqueous solution by a process called evaporation. Simply heat the solution to evaporate the water, leaving behind solid KNO3. This method exploits the fact that KNO3 has a much higher boiling point compared to water.
Compare the boiling and freezing points of 1m solution of glucose to a 1m solution of Cacl2. Why does CaCl2 have a higher boiling and a lower freezing Please explain not just say its 1m and then 3m?
A 1M solution of glucose will have higher boiling and freezing points compared to a 1M solution of CaCl2. This is because CaCl2 dissociates into three ions (1 Ca2+ and 2 Cl-) per formula unit in solution, leading to a higher boiling point due to increased colligative properties. Additionally, the presence of more solute particles hinders the formation of a solid lattice structure, resulting in a lower freezing point.
