Calculate the Molarity of a Solution

What is the molarity of a solution containing 15.6 g of KCl in 274 ml of KCl solution?

Answer:

The molarity of a solution containing 15.6 g of KCl in 274 ml is approximately 0.763 M.

Calculating the molarity of a solution involves converting the mass of the solute to moles and the volume of the solution to liters. Molarity (M) is defined as the number of moles of solute per liter of solution.

First, the mass of KCl is converted to moles using the molar mass of KCl, which is approximately 74.55 g/mol. Therefore, 15.6 g of KCl is equal to 15.6 g / 74.55 g/mol = 0.209 moles.

Next, the volume of the solution is converted from milliliters to liters. 274 ml is equivalent to 274 ml / 1000 = 0.274 liters.

Finally, the molarity is calculated by dividing the number of moles of solute by the volume of solution in liters. This gives 0.209 moles / 0.274 liters = 0.763 M, so the molarity of the solution is approximately 0.763 M.