chemistry

posted by .

prepare 1M 100 ml H2SO4. 98% H2SO4, density 1.84

  • chemistry -

    First of all, the density makes no sense without units. Secondly, you should only specify the amount of something present in one way. The questions gives two: (1) a molarity and a volume. (2) a percentage (by volume or by mass?) and a density. So you can't solve such a question unambiguously in general.

    Suppose we go with the given molarity. That means there are 0.1 moles of sulfuric acid present (1.0 mol/L * 0.1 L). That will require adding how many grams to 100 mL of water? Molecular mass of H2SO4 = 98 g/mol, so use 98*0.1 = 0.98 grams of H2SO4.

    If we go with the percent by mass, then assume the density was supposed to be 1.84 g/L, then that's 1.84g/L*0.1L = 0.184 grams all told, 98% of which is H2SO4 = 0.18032 grams.

    So you see, the desired solution is impossible to obtain on the face of it. You can either have a desired molarity or a desired mass percentage and density, but not both (unless by luck the desired quantities coincide).

  • chemistry -

    First of all density with no units is meaningless and makes the question impossible to solve.

    Secondly the percentage without the type is meaningless.
    Although can easily be find out in such question but, you should be specify that.

    But to give idea about the solution lets assume
    d(H2SO4) = 1.84 kg/L and 98% means
    100 unit volume of stock solution contains
    98 unit volume of H2SO4

    so problem asks us to find the amount (mL) of H2SO4 (stock) to prepare 100 mL of 1M soluiton


    x mL stock(H2SO4) =
    (1mol H2SO4 / 1L solution) *
    (1L solution / 1000mL solution) * (100mL solution) *
    (98.04g H2SO4 / 1mol H2SO4) *
    (1kg H2SO4 / 1000 g H2SO4) *
    (1L H2SO4 / 1.84kg H2SO4) *
    (1000mL H2SO4 / 1L H2SO4) *
    (100ml stockH2SO4 / 98mL H2SO4)

    ----
    x mL H2SO4 = 5.437 mL

    to prepare 100 mL, 1M H2SO4 from stock (98% [v/v]; 1.84 [kg/L]; 98.04 [g/mol])

    to 100 mL flat bottom flask add some amount of water (not much),
    and pour 5.45 mL H2SO4 stock solution on it.
    Dilute the solution to 100 mL

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. science

    Concentrated sulfuric acid (18.4 molar H2SO4) has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar, the solution has a density of 1.38 grams per milliliter and can be used as an electrolyte in lead storage …
  2. Chemistry pls help

    I have a chemistry question Please advise how do I prepare 1L of 75% H2SO4 from concentrated H2SO4 (98% of density 1.84g/ml)?
  3. bio chemistry

    prepare 1M 100 ml H2SO4, density 1.84
  4. bio chemistry (please help)

    prepare 1M 100 ml H2SO4. 98% H2SO4, density 1.84
  5. Chemistry

    Calculate the volume of concentrated reagent required to prepare the diluted solutions indicated: (a) 18 M H2SO4 to prepare 225 mL of 2.0 M H2SO4 (
  6. chemistry

    Consider 18.0 M H2SO4, if you need to make 250.0 mL of a 3.0 M solution of H2SO4, how would you do this?
  7. Chemistry

    Consider 18.0 M H2SO4, if you need to make 250.0 mL of a 3.0 M solution of H2SO4, how would you do this?
  8. Chemistry

    What volume of 5.0 M H2SO4 should be diluted to 100mL to prepare a 0.25 M H2SO4 M solution?
  9. Chemistry

    My chemistry is bad. I know these are very easy but I cannot solve them . 1. a) Prepare 200 ml of 2 M HCl solution from stock bottle containing 37% w/w HCl and d = 1.2 (g/ml). MWHCl = 36.5 g b) Calculate M of 37% w/w HCl solution?
  10. Chemistry

    h2so4 is labelled as 9.8 by weight. specific gravity of h2so4 is 1.8. the volume of acid to be taken to prepare 100 ml of 0.18M solution is?

More Similar Questions