Which aqueous solution freezes at the lowest temperature

Which of the following aqueous solutions would have the lowest freezing point? Calculate the number of moles of solute present in each of the following aqueous solutions: a mL of 0.

Which aqueous solution will have the lowest freezing point? Which of the following aqueous solutions has the lowest vapor pressure at a given temperature? Which of the following solutions has the lowest boiling point? Create an Account and Get the Solution. Log into your existing Transtutors account.

Have an account already? Click here to Login. No Account Yet? Social studies. Ben Davis April 12, What is the freezing point of an aqueous solution? What is the freezing point of glucose? What is the boiling point of an aqueous solution that freezes at?

What is the boiling point of an aqueous solution that freezes at KF 1. How do you find the boiling point of aqueous solution?

Which aqueous solution has the highest boiling point? Which aqueous solution has the lowest freezing point? Which of the following aqueous solution has maximum freezing point? Which aqueous solution will have the lowest boiling point temperature? Which of the following solution will have the lowest boiling point?

Which solution would you expect to have the lowest boiling point? Which compound has the lowest melting point? What is the normal boiling point for CCl4? Which compound has lower boiling point?

Do double bonds increase boiling point? Which solution has maximum freezing point? The freezing point depression is the difference in the freezing points of the solution from the pure solvent. This is true for any solute added to a solvent; the freezing point of the solution will be lower than the freezing point of the pure solvent without the solute. Thus, when anything is dissolved in water, the solution will freeze at a lower temperature than pure water would.

The freezing point depression due to the presence of a solute is also a colligative property. That is, the amount of change in the freezing point is related to the number of particles of solute in a solution and is not related to the chemical composition of the solute.

Recall that covalent and ionic compounds do not dissolve in the same way. Ionic compounds break up into cations and anions when they dissolve. Covalent compounds typically do not break up. Remember that colligative properties are due to the number of solute particles in the solution. Adding 10 molecules of sugar to a solvent will produce 10 solute particles in the solution. Colligative properties depend on the number of solute particles in the solution.

By knowing the molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict which solution in a group will have the lowest freezing point.

To compare the boiling or freezing points of solutions, follow these general steps:. Rank the following solutions in water in order of increasing lowest to highest freezing point:. To compare freezing points, we need to know the total concentration of all particles when the solute has been dissolved.

Remember, the greater the concentration of particles, the lower the freezing point will be. The boiling point of a solution is higher than the boiling point of a pure solvent, and the freezing point of a solution is lower than the freezing point of a pure solvent. However, the amount to which the boiling point increases or the freezing point decreases depends on the amount of solute that is added to the solvent.

A mathematical equation is used to calculate the boiling point elevation or the freezing point depression. The boiling point elevation is the amount that the boiling point temperature increases compared to the original solvent. The freezing point depression is the amount that the freezing temperature decreases. Both the boiling point elevation and the freezing point depression are related to the molality of the solution.

Looking at the formula for the boiling point elevation and freezing point depression, we see similarities between the two. The equation used to calculate the increase in the boiling point is:.