Question

500.0 mL of 0.20 M phosphoric acid is

added to 1.00 L of water. What is the
molarity of the resulting solution?

Answer 1

Step-by-step explanation:

When the 500.0 mL of 0.20 M phosphoric acid is added to 1.00 L of water, the total volume of the resulting solution becomes:

500.0 mL + 1000.0 mL = 1500.0 mL = 1.5 L

The number of moles of phosphoric acid in the solution is:

moles of H3PO4 = Molarity × volume in liters

moles of H3PO4 = 0.20 M × 0.500 L = 0.100 mol

The molarity of the resulting solution is then:

Molarity = moles of solute ÷ volume of solution in liters

Molarity = 0.100 mol ÷ 1.5 L = 0.067 M

Therefore, the molarity of the resulting solution is 0.067 M.