chemistry

Commercially available concentrated sulfuric acid is 18.0 M H2SO4. Calculate the volume (in mL) of concentrated sulfuric acid required to prepare 1.60 L of 0.320 M H2SO4 solution.

  1. 👍 0
  2. 👎 0
  3. 👁 604
  1. mL x M = mL x M

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Gen Chem 1

    A tanker truck carrying 2.01×10^3kg of concentrated sulfuric acid solution tips over and spills its load. The sulfuic acid is 95.0% H2SO4 by mass and has a density of 1.84g/L. Sodium Carbonate (Na2CO3)is used to neutralize the

  2. chemistry

    commercially available concentrated hydrochloric acid is 37.0% w/w HCl. Its density is 1.18 g/mL. Using this information calculate (a) the molarity of concentrated HCl, and (b) the mass and volume (in mL) of solution containing

  3. chemistry

    commercially available concentrated Hydrochloric acid is 37.0% w/w Hcl.its density is 1.18g/ml.using this information calculate (a)the molarity of concentrated Hcl,and (b)the mass and volume (in ml)of solution containing 0.315 mol

  4. Chemistry

    Ca3(PO4)2 + 3 H2SO4 -> 3 CaSO4 + 2 H3PO4 What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H2SO4 by mass)?

  1. 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 (

  2. chemistry

    A flask has a mass of 78.23 g when empty and 593.63 g when filled with water. When the same flask is filled with concentrated sulfuric acid, H2SO4, its mass is 1026.57 g. What is the density of concentrated sulfuric acid? (Assume

  3. Chemistry!!

    A chemist wants to prepare a stock solution of H2SO4 so that a sample of 20.00mL will produce a solution with a concentration of .50 M when added to 100.0mL of water. A)what should the molarity of the stock solution be? B)If the

  4. Chemistry

    Concentrated sulfuric acid is 18.4 molar and 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. This concentration of H2SO4 is often used in

  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

  2. Chemistry

    A solution is prepared by adding 50.3 mL of concentrated hydrochloric acid and 16.6 mL of concentrated nitric acid to 300 mL of water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for

  3. AP Chemistry

    Sulfuric acid (H2SO4)is prepared commercially from elemental sulfur using the contactprocess. In a typical sequence of reactions,the sulfur is first burned:S + O2→SO2,then it is converted to SO3 using a

  4. chemistry

    how would you prepare 1.00 L of a .50M solution of H2SO4 from concentrated (18M) sulfric acid?

You can view more similar questions or ask a new question.