Ask Question
19 July, 14:37

A solution is prepared by dissolving 0.5636 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the diluted oxalic acid solution

+3
Answers (1)
  1. 19 July, 14:58
    0
    The final molarity of the diluted oxalic acid solution is 0.002504 M

    Explanation:

    Step 1: Data given

    Mass of oxalic acid (H2C2O4) = 0.5636 grams

    Volume of the solution = 100.0 mL = 0.100 L

    A 10 ml of this solution diluted in 250 ml of solution.

    Molecular weight of H2C2O4 = 90.03 g/mol

    Step 2: Calculate initial moles of H2C2O4

    Moles H2C2O4 = mass / molar mass

    Moles H2C2O4 = 0.5636 grams / 90.03 g/mol

    Moles H2C2O4 = 0.00626 moles

    Step 3: Calculate molarity of the solution

    Molarity = moles / volume

    Molarity = 0.00626 moles / 0.100 L

    Molarity = 0.0626 M

    Step 4: Calculate moles of a 10.00 mL aliquot

    Moles = 0.0626 M * 0.010 L

    Moles = 0.000626 moles

    Step 5: Calculate the new molarity

    Molarity = 0.000626 moles / 0.250 L

    Molarity = 0.002504 M

    The final molarity of the diluted oxalic acid solution is 0.002504 M
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “A solution is prepared by dissolving 0.5636 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers