Why is the freezing point of 0.1 m NaCl?
Answer: 0.1M NaCl and0. … The depression in freezingpoint is inversly proprotional to molar mass of solute thus more is molar mass of solute lesser is the depression in freezing point . Thus it can explain that the NaCl wil be more than the glucose.
Does NaCl have the lower freezing point?
The actual reason that the application of salt causes ice to melt is that a solution of water and dissolved salt has a lower freezing point than pure water. … The higher the concentration of dissolved salt, the lower its overall freezing point.
What is the freezing point of an aqueous 1.00 M NaCl solution?
The freezing points of solutions are all lower than the pure solvent and also it is directly proportional to molality of the solute. Thus, the freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water is\[-{{3.72}^{o}}C\].
What will be the freezing point depression of 0.4 m NaCl solution and 0.4 m glucose solution?
According to Van't Hoff, Van't Hoff factor for\[NaCl\] is 2 and for glucose, it is 1. Van't Hoff factor is more means freezing point depression is more. So, the freezing point depression (\[\Delta {{T}_{f}}\]) of 0.4 M \[NaCl\] solution is nearly twice that of 0.4 M Glucose solution.
Why is freezing point depression of 0.1 m NaCl solution is nearly twice that of 0.1 glucose solution?
Answer: Freezing point depression of 0.1m nacl solution nearly twice that of 0.1m glucose solution because NaCl is a strong electrolyte and it dissociates to give two ions and , whereas glucose is a non electrolyte and it does not dissociate to give ions.
Does saline freeze?
saline solution is necessarily above 0° C and stays at 0° C after it freezes. 2. Such temperatures are relatively safe for living tissues.
How do you find the freezing point in chemistry?
The freezing point depression ∆T = KF·m where KF is the molal freezing point depression constant and m is the molality of the solute. Rearrangement gives: mol solute = (m) x (kg solvent) where kg of solvent is the mass of the solvent (lauric acid) in the mixture.
What is the freezing point of .5 m NaCl AQ?
A solution's molality will tell you how many moles of solute you get per kilogram of solvent. In this case, the only information you have is that a given sodium chloride solution has a freezing point of −5.58∘C .