# Assuming 100% dissociation, what is the freezing point and boiling point of 3.39 m #K_3PO_4(aq)#?

To do this, we can use the equations

where

Plugging in known values, we have

These are by how much the freezing and boiling point temperatures decrease (freezing point) and increase (boiling point).

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The freezing point depression and boiling point elevation formulas can be used to calculate these values.

For the freezing point depression: ΔTf = -i * Kf * m

For the boiling point elevation: ΔTb = i * Kb * m

Where:

- i is the van't Hoff factor, which represents the number of particles formed per formula unit dissolved. For K3PO4, i = 4 because it dissociates into 4 ions (3 K+ ions and 1 PO4^3- ion).
- Kf is the cryoscopic constant and Kb is the ebullioscopic constant for the solvent.
- m is the molality of the solution.

Given that K3PO4 dissociates completely, the molality of the solution is equal to the concentration of K3PO4 in moles per kilogram of solvent.

You would need to know the values of Kf and Kb for the solvent in order to calculate the freezing point depression and boiling point elevation, respectively. These values depend on the specific solvent being used.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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