Question

Calculate the volume, in liters, of a 0.29 m Barium Chlorate Ba(CIO₃)₂ solution that contains 150 g of barium chlorate. Be sure your answer has the correct number of significant digits.

Answer 1

First, convert 150 g of Ba(ClO₃)₂ to moles using its molar mass, then divide the moles by the molarity (0.29 M) to find the volume. The result is reported with two significant digits, yielding 1.7 liters.

Step-by-step explanation:

To calculate the volume of a 0.29 M Barium Chlorate Ba(ClO₃)₂ solution that contains 150 g of barium chlorate, we must first convert the mass of barium chlorate to moles. The molar mass of Ba(ClO₃)₂ is Ba + 2 x (Cl + 3 x O) = 137.33 + 2 x (35.45 + 3 x 16) = 137.33 + 2 x (35.45 + 48) = 137.33 + 2 x 83.45 = 304.23 g/mol. So, we calculate the number of moles of barium chlorate in 150 g:

moles = mass / molar mass = 150 g / 304.23 g/mol = 0.493 moles

Since the solution concentration is 0.29 M (moles/liter), we can find the volume by dividing the number of moles by the concentration:

volume = moles / concentration = 0.493 moles / 0.29 M = 1.70 liters

The volume should be reported with two significant digits, which matches the number of significant digits in the given molarity (0.29 M). Therefore, the final answer is 1.7 liters.