Molar Concentration: Understanding the Chemistry Behind It

What is the concentration in molarity of an aqueous solution which contains 5.06% by mass ethylene glycol?

The concentration in molarity of an aqueous solution containing 5.06% by mass ethylene glycol is 0.847 mol/L.

Molar concentration, commonly referred to as molarity, is a crucial concept in chemistry that measures the amount of a chemical species (usually a solute) per unit volume of solution. In this case, we are determining the molar concentration of an aqueous solution that contains 5.06% by mass of ethylene glycol.

To calculate the molarity of the solution, we first need to determine the amount of ethylene glycol present. Using the given data, we can calculate that the molar mass of ethylene glycol (C2H6O2) is 62.07 g/mol and the mass of ethylene glycol is 0.0506 g.

By dividing the mass of ethylene glycol by its molar mass, we can determine the number of moles of ethylene glycol present in the solution, which is 8.154 E-4 mol.

Next, we calculate the volume of the solution by dividing the mass of the solution (1g) by its density (1.04 g/mL), resulting in a volume of 9.615 E-4 L.

Finally, we calculate the molarity by dividing the number of moles of ethylene glycol by the volume of the solution, which gives us a molarity of 0.847 mol/L.

In summary, molarity is a vital measure of the concentration of a chemical species in a solution, expressed in moles per liter. It provides valuable insights into the amount of material present per unit volume of solution, allowing chemists to accurately quantify the concentration of solutes in a solution.

To delve deeper into the concept of molarity and its significance in chemistry, you can explore the link provided for a more in-depth explanation.