**Molality is the ratio between the amount of matter in a solute (in moles - n _{1}) by the mass in kilograms of the solvent (m_{2}).**

The symbol of molality is usually the **W** and it can be calculated by the following formula:

**W = no_{1}m_{2}**

Molality can also be called **concentration in quantity of matter per mass** or **molal concentration**.

**Mind Map - Mol**

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See an example of how to perform this calculation:

“Calculate the molality of a solution that was prepared by dissolving 126.0 g of nitric acid (HNO_{3}) in 2.0 liters of water, whose density is equal to 1.0 g/mL. The molar mass of nitric acid is equal to 63.0 g/mol.”

First, we need to find the values of n._{1} and of m_{2}:

no_{1} = __m _{1}__

M

_{1}

no

_{1}=

__126.0 g__

63.0 g/mol

no

_{1}= 2.0 mol

We can find out the value of the mass of the solvent (m_{2}) through the density formula:

d = __m__ → m = d. v → m_{2} = (1.0 g/ml). (2000 mL) → m_{2} = 2000 g or 2.0 kg of water

v

Now we can replace the values in the molality formula:

W = __no _{1}__

m

_{2}

W =

__2.0 mol__

2.0 kg

**W = 1.0 mol/kg**or

**1.0 mole**

In cases where there is 0.1 mol of solute or less dissolved in 1 liter of solution, the molality value will be practically equal to the molarity value (or concentration in mol/L).

Currently, this quantity is practically not used, but since its formula does not involve the value of the volume of the solution, which can vary with temperature, it is very useful to use when the temperature of the solution in question vary. It can also be useful in the study of colligative properties.

*** Mind Map by Me. Diogo Lopes**

By Jennifer Fogaça

Graduated in Chemistry