Question

determine the molarity of a solution that is made by dissolving 20.0 g of ammonium nitrate, NH₄NO₃, in enough water to make 250.0 ml of solution.

Answer 1

The molarity is M = (0.24994 mol) / (0.250 L) = 0.99976 M

Step-by-step explanation:

To determine the molarity of the solution, we need to first calculate the number of moles of NH₄NO₃ in the solution. We can do this by using the molar mass of NH₄NO₃, which is the sum of the atomic masses of its elements.

Molar mass of NH₄NO₃ = 14.01 g/mol (mass of N) + 4(1.01 g/mol) (mass of H) + 3(15.99 g/mol) (mass of O) = 80.04 g/mol.

Next, we can use the formula for molarity (M) to calculate the molarity of the solution:

• M = (moles of solute) / (volume of solution in liters).

In this case, we have:

• Mass of NH₄NO₃ = 20.0 g

• Molar mass of NH₄NO₃ = 80.04 g/mol

• Volume of solution = 250.0 mL = 0.250 L

Using these values, we can calculate the moles of NH₄NO₃:

• moles of NH₄NO₃ = (20.0 g) / (80.04 g/mol) = 0.24994 mol.

Finally, we can calculate the molarity:

• M = (0.24994 mol) / (0.250 L) = 0.99976 M