Chemistry

How much concentrated solution would you take to prepare 2.80L of 0.475M HCl by mixing with water?

Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20g/mL.

  1. 👍 0
  2. 👎 0
  3. 👁 1,836
  1. Calculate the molarity of the concd HCl.
    1.20 g/mL x 1000 mL x 0.37 x (1/36.5) = about 12 M or so but you do it exactly.

    Then mL x M = mL x M
    mL x 12 M = 2800 mL x 0.475
    Solve for mL of the concd HCl solution.

    1. 👍 1
    2. 👎 0
  2. Hey thank you DrBob222! That really helped!

    1. 👍 1
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    How do I prepare 100mL of 10g/L HCl from concentrated HCl(37%HCl, density 1.19g/mL) Is it 2.28mL of conc HCl dilute to 100mL with water? Please show the calculation steps.

  2. chem

    A sample of 7.80L of NH3 (ammonia) gas at 22 degrees and 735mmHg is bubbled into a 0.350L solution of 0.400M HCL(hydrochloric acid). The Kb value for NH3 is 1.8x10-5 Assuming all the NH3 dissolves and that the volume of the

  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

    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

  1. chemistry

    The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is i solved it but my answer is wrong. the right one is 1.97. am i missing a step? moles of HCl left over = (moles of HCl) – ( moles of KOH)

  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

    Aqueous ammonia is commercially available at a concentration of 16.0 M. Part A How much of the concentrated solution would you use to prepare 500.0mL of a 1.30M solution?

  4. science

    Describe the preparation of 100 mL of 6.0 M HCL from a concentrated solution that has a specific gravity of 1.18 and is 37% (w/w) HCL

  1. chemistry

    Hydrochloric acid is usually purchased in concentrated form with a 37.0% HCL concentration by mass and a density of 1.20g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5L of 0.500M HCL

  2. Chemistry

    You can purchase hydrochloric acid in a concentrated form that is 37.0 hcl by mass and has a density of 1.20g/mL. Describe how exactly you would prepare 2.85 L of 0.500 M HCL from the concentrated solution.

  3. 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

  4. Chemistry

    1) Prepare 100mL of 10%w/w HCl from 37%concentrated HCl(density of 37%HCl =1.19g/ml) 2) Prepare 100mL of 10%w/v HCl from 37% concentrated HCl(density of 37%HCl=1.19g/ml) Can you please show the calculation steps for 1) & 2)? Is

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