Ask Question
2 June, 11:38

The student diluted 50.00 mL of commercial bleaching solution to 250 mL in a volumetric flask, and titrated a 20-mL aliquot of the diluted bleaching solution. The titration required 35.46 mL of 0.1052M Na2S2O3 solution. A faded price label on the gallon bottle read $0.79. The density of the bleaching solution was 1.10 g/mL

Determine the volume of commercial bleaching solution present in the diluted bleaching solution titrated

+4
Answers (1)
  1. 2 June, 13:13
    0
    To get the volume of the original solution in the dilution, we consider the dilutions that were made:

    from 50 mL to 250 mL:

    1/5 of original was present

    from 20 mL of 250 mL:

    1/12.5 of the diluted mixture was presetn

    So, V=50 mL * (1/5) * (1/12.5) = 0.8 mL of original bleaching solution was present in dilution
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “The student diluted 50.00 mL of commercial bleaching solution to 250 mL in a volumetric flask, and titrated a 20-mL aliquot of the diluted ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers