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What is the boiling point of glucose dissolved in water?
The boiling point of a solution can vary depending on the concentration of solute. For a dilute solution of glucose in water, the boiling point elevation is typically small and may not be easily measurable. However, pure glucose itself does not have a defined boiling point as it decomposes upon heating.
What is the boiling point of a 2.47 molal solution of napthalene in benzenethe boiling point of benzene is 80.1?
To determine the boiling-point elevation of the solution, we need to use the formula: ΔTb = iKbm, where ΔTb is the boiling point elevation, i is the van't Hoff factor (for napthalene, i = 1 because it doesn't dissociate), Kb is the ebullioscopic constant of the solvent (benzene), and m is the molality of the solution (2.47 mol/kg). Plug in the values and solve for ΔTb. Add this value to the boiling point of benzene (80.1°C) to find the boiling point of the solution.
Boiling point of 1 omol solution of sugar?
The boiling point of a 1 molal (1 m) solution of sugar will be higher than that of pure water because sugar is a non-volatile solute that elevates the boiling point of the solution through boiling point elevation. The exact boiling point elevation can be calculated using the formula: ΔTb = i * Kf * m, where i is the van't Hoff factor, Kf is the cryoscopic constant of the solvent, and m is the molality of the solution.
What is the boiling point of a solution of 0.10 mole of glucose in 200ml of water?
To determine the boiling point of a solution of glucose in water, we first calculate the molality of the solution. With 0.10 moles of glucose in 200 mL of water (approximately 0.2 kg), the molality is 0.5 mol/kg. The boiling point elevation can be calculated using the formula ΔT_b = i * K_b * m, where K_b for water is 0.512 °C kg/mol. Thus, the boiling point elevation is approximately 0.26 °C, raising the boiling point of water from 100 °C to about 100.26 °C.
What is the change in the boiling point and freezing point of 500 grams of water if 45 grams of glucose C6H12O6 were dissolved in it?
This quantity is equivalent to 90 g glucose / kg water = 0.50 mole particles of solute / kg water, so with a 'molar cryoscopic constant' for water of -1.86 oC/kgthis lowers the freezing point to -0.93 oC.
What is the experimentally determined concentration of particles for an 2.25 molal solution of an ionic substance in water if the boiling point of the solution is 100.3 oC?
The experimentally determined concentration of particles for a 2.25 molal solution can be calculated using the formula: ΔTb = i * Kf * molality, where ΔTb is the boiling point elevation, i is the Van't Hoff factor, Kf is the ebullioscopic constant for water (0.512 oC/kg/mol), and molality is 2.25 mol/kg. From the given values, you can solve for the Van't Hoff factor (i) to determine the concentration of particles in the solution.
Which solution would elevate the boiling point of water the most MgF2 glucose KNO3 KBr?
MgF2
Calculate the boiling point of a solution of 10 grams of sodium chloride in 200 grams of water?
The boiling point elevation is determined by the molality of the solution, which can be calculated as the moles of solute divided by the mass of solvent in kg. From there, you can use the van't Hoff factor and the molal boiling point elevation constant to determine the change in boiling point. For sodium chloride, the van't Hoff factor is 2. The boiling point elevation constant for water is approximately 0.51 degrees Celsius/m.
Why does the KCI solution have the higher boiling point if in a experiment 1 mol KCLid dissolved in a 1.4 kg sample of waater the 1mol glucose ids dissolved i another 1.4kg sample of water?
The KCl solution has a higher boiling point than the glucose solution due to the presence of ions. KCl dissociates into potassium (K⁺) and chloride (Cl⁻) ions in solution, effectively increasing the number of solute particles (colligative properties). In contrast, glucose does not dissociate and remains as intact molecules, resulting in fewer solute particles. This increase in particle concentration in the KCl solution elevates its boiling point through boiling point elevation.
What is the boiling point of water glucose?
The boiling point of water is 100 degrees Celsius. Glucose, on the other hand, does not have a fixed boiling point because it decomposes before reaching a boiling point.
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.
How a solute affects the boiling point of a solution?
The addition of a non-volatile solute elevates the boiling point of a solution (in addition to the depression of freezing point). The formula is ΔT = Kbm where ΔT is the change in temperature, Kb is the ebullioscopic constant, and m is the molality (not molarity) of the solution.
