An antifreeze solution is prepared from \(222.6 \mathrm{~g}\) of ethylene glycol \(\left[\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{OH})_{2}\right]\) and \(200 \mathrm{~g}\) of water. Calculate the molality of the solution. If the density of the solution is \(1.072 \mathrm{~g} \mathrm{~mL}^{-1}\) then what shall be the molarity of the solution?

Molality, often denoted as 'm', is a measure of the concentration of a solute in a solution. Specifically, it refers to the number of moles of solute per kilogram of solvent. Unlike molarity, molality is not affected by temperature changes because mass doesn't change with temperature.

To calculate molality, you first need to find the number of moles of the solute, which can be done by dividing its mass by its molar mass. Then, you divide the moles of solute by the mass of the solvent in kilograms. For instance, in the antifreeze example provided, you would divide the mass of ethylene glycol by its molar mass to find its moles and then divide by the mass of water in kilograms.

Molarity, represented by 'M', is another way to describe the concentration of a solution. It is defined as the number of moles of solute divided by the volume of the solution in liters. Unlike molality, molarity is temperature-dependent because volume can change with temperature.

When calculating molarity, as in the antifreeze example, you'll first ascertain the total number of moles of the solute. Then you calculate the volume of the solution using its total mass and the given density. Finally, you'll divide the number of moles of solute by this volume in liters. This gives you the molarity of the solution, allowing you to understand how concentrated the solute is within the total volume of the solution.

The concentration of a solution is a measure of how much solute is dissolved in a given quantity of solvent or solution. There are various ways to express this, with molality and molarity being two of them.

The concentration can affect properties like boiling point, freezing point, and vapor pressure. It's important in various applications, from industrial processes to biological systems. When preparing solutions in a lab or industry, precise calculations of concentration are essential to ensure reactions proceed correctly or products meet quality standards.

Chemical calculations are used to quantify substances and their changes during chemical reactions. When dealing with solutions, we often need to calculate quantities like the number of moles, molarity, and molality to name a few.

These calculations require a solid understanding of concepts like molar mass, Avogadro's number, and the relationships between units of mass, volume, and moles. They are pivotal for preparing solutions of precise concentrations, predicting the outcome of reactions, and scaling up processes from the lab to industrial production.