Question

In the laboratory you dissolve 22.9 g of ammonium acetate in a volumetric flask and add water to a total volume of 375 mL.

What is the molarity of the solution?
a. 0.5 M
b. 1.0 M
c. 0.6 M
d. 0.3 M

Answer 1

To find the molarity, divide the number of moles of ammonium acetate (22.9 g / 77.08 g/mol) by the volume of the solution in liters (0.375 L). The calculated molarity is 0.792 M, which suggests a potential mistake in the options provided.

Step-by-step explanation:

To calculate the molarity of the solution, we first need to know the number of moles of ammonium acetate that are being dissolved. Since we know that the mass of ammonium acetate is 22.9 g and the molar mass is 77.08 g/mol, we can find the moles by dividing the mass by the molar mass:

Moles of ammonium acetate = 22.9 g / 77.08 g/mol = 0.297 moles

Next, we need to convert the volume of the solution from milliliters to liters in order to use it in the molarity calculation. As there are 1000 milliliters in a liter, we have:

375 mL = 0.375 L

Finally, the molarity (M) is calculated by dividing the number of moles of solute by the liters of solution:

Molarity (M) = 0.297 moles / 0.375 L = 0.792 M

The nearest option to 0.792 M would be option (c) 0.6 M, as this is a multiple choice question. However, it's crucial to note that the result obtained here does not match any of the options provided exactly. Therefore, there might have been a mistake in the calculation, the options provided, or the initial values given in the problem.