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The k3po4 boiling point is the temperature increase in an aqueous solution that occurs when a liquid is diluted with water. Boiling point elevation and freezing point depression are colligative properties that are determined by the proportion of solute particles to solvent particles in the solution.

Typical solutions of potassium phosphate are alkaline and have pHs of 11.5-12.3. The phosphate ion is very important in cells and plays an important role in energy storage. It is used as a base in organic chemistry reactions and can also function as an accelerator or catalyst.

Insoluble in ethanol, very soluble in water at 25 degC and forms alkaline solutions. A 1% K3PO4 solution in water has a pH of 11.5-12.3.

When dissolved in water, K3PO4 separates into three potassium ions and a phosphate ion PO43-. The phosphate ion takes one proton from the water and the hydrogen phosphate anion HPO is formed. The aqueous solution becomes alkaline, with many OH ions.

Using this knowledge, we can calculate the change in freezing point and boiling point of a 3.39m solution of K3PO4. It must completely ionize and so the equation for freezing point depression is: Tf = DTf + i * e.

Similarly, the calculation for boiling point elevation is Tb = DTb + i * m* Kb. To use the calculator, choose a solvent from the list and enter the molality of the solution. The ebullioscopic constant and Van’t Hoff factor can then be entered. The change in freezing point and boiling point can then be calculated by multiplying the morality of the solution with the ebullioscopic constant and Van’t-Hoff factor to get the temperature increase or decrease.