What are the boiling point and freezing point of a 0.516 m aqueous solution of any nonvolatile, nonelectrolyte solute?

Explanation:

1. Boling point

The boiling point of a solvent will increase when a solute is added. The boiling point elevation is a colligative property.

When a nonvolatile, nonelectrolyte solute is added to a solvent, the increase of the boiling point may be calculated using the formula:

Where m is the molality and Kb is the the molal boiling point constant (for water, Kb = 0.512ºC/m ).

Substitute and compute:

Hence, add the increase in the boiling point to the normal boiling point of water: 100.000ºC

2. Freezing point

The freezing point of a solve will decrease when a solute is added. The depression on the freezing point is another colligative property.

When a nonvolatile, nonelectrolyte solute is added to a solvent, the depression of the boiling point may be calculated using the formula:

Where m is the molality and Kf is the the molal freezing point constant (for water, Kf = 1.86 ºC/m ).

Substitute and compute:

Subtract the decrease on the freezing point from the normal freezing point of water: 0.000ºC

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8