Ask Question
29 July, 08:50

Nitric acid is usually purchased in concentrated form with a 70.3% HNO3HNO3 concentration by mass and a density of 1.41 g/mLg/mL. Part A How much of the concentrated stock solution in milliliters should you use to make 2.0 LL of 0.500 MM HNO3HNO3?

+4
Answers (1)
  1. 29 July, 09:47
    0
    V = 63.57 mL

    Explanation:

    In this case, to get the mL of the stock nitric acid we need to know first the concentration in mol/L so it can match the units of the desired concentration, in this case, 0.5 mol/L

    To get the concentration of the stock solution, we should use the following expression:

    M = % * d * 1000 / MM * 100

    The molar mass of the nitric acid (HNO₃) is:

    MM = 1 + 14 + 3 (16) = 63 g/mol

    the concentration of the acid is:

    M = 70.3 * 1.41 * 1000 / 63 * 100

    M = 15.73 M

    Now that we know the concentration of the solution, we use the following expression to get the volume:

    M1*V1 = M2*V2

    Replacing the values and solving for V1 we have:

    V1 = M2*V2 / M1

    V1 = 2 * 0.5 / 15.73

    V1 = 0.06357 L

    In mL it will be:

    V1 = 0.06357 * 1000 = 63.57 mL
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Nitric acid is usually purchased in concentrated form with a 70.3% HNO3HNO3 concentration by mass and a density of 1.41 g/mLg/mL. Part A ...” 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