Ask Question
30 May, 04:40

If all of the chloride in a 4.106-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO3, what is the percentage of chloride in the sample?

+4
Answers (1)
  1. 30 May, 08:14
    0
    The chloride is precipitated as following:

    AgNO₃ + Cl⁻ → AgCl + NO₃⁻

    molar concentration = number of moles / solution volume

    number of moles = molar concentration * solution volume

    number of moles of AgNO₃ = 0.2010 * 70.90

    number of moles of AgNO₃ = 14.25 mmoles

    from the equation

    if 1 mmole of AgNO₃ is needed to precipitate 1 mmole of chloride

    then 14.25 mmoles of AgNO₃ are needed to precipitate X mmoles of

    chloride

    X = 14.25 mmoles of choride

    mass = number of moles * molecular weight

    mass of chloride = 14.25 * 35.5

    mass of chloride = 505.9 mg = 0.5059 g

    if in 4.106 g of sample we have 0.5059 g of chloride

    then in 100 g of sample we have X g of chloride

    X = (100 * 0.5059) / 4.106 = 12.32 % chloride
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “If all of the chloride in a 4.106-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO3, what is ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers