Question

What is the molarity of sodium sulfate if 10.56 g BaSO₄ is precipitated from 500 mL of Na₂SO₄?

a) 0.18 M
b) 0.18 m
c) 0.09 M
d) 0.09 m

Answer 1

The molarity of sodium sulfate in the solution is approximately 0.148 M.

Step-by-step explanation:

To find the molarity of sodium sulfate in the solution, we need to use the equation:

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

First, we need to calculate the moles of sodium sulfate. The molar mass of Na₂SO₄ is 142.04 g/mol. We can use the given mass (10.56 g) and molar mass to find the number of moles:

Moles = mass / molar mass = 10.56 g / 142.04 g/mol ≈ 0.0743 mol

Next, we need to convert the volume of the solution to liters:

Volume = 500 mL = 500/1000 L = 0.5 L

Finally, we can calculate the molarity:

Molarity = moles of solute / volume of solution = 0.0743 mol / 0.5 L ≈ 0.148 M

Therefore, the molarity of sodium sulfate in the solution is approximately 0.148 M.