Chemistry

posted by .

You have an unlimited amount of 12M HCl stock solution. You need to neutralize 2.00 grams of NaOH by slowly adding 0.100M HCl solution. How will you prepare the proper amount of hydrochloric acid solution to add to the beaker of sodium hydroxide using a 500 ml volumetric flask.

  • Chemistry -

    2.00 g = 2.00/molar mass NaOH = about 0.05 moles NaOH and that will take 0.05 moles HCl.

    mL12M x M12M = mL0.1M x M0.1M
    mL x 12 = 500 x 0.1
    mL of 12M acid = (500 x 0.1/12) = 4.167.
    I would use a 5.000 mL buret, add exactly 4.167 mL of the 12M stock solution of HCl to the 500 mL volumetric flask, then add DI or distilled water to the mark of the flask and mix thoroughly.

    (As extra information, I provide the follwing. For whatever it's worth, I would do it a different way and use a 4 mL pipet, transfer exactly 4.00 mL with a pipet to the flask and proceed. That will NOT make 0.1M; the concn will be 0.096 but that's much simpler. Four mL pipets are easily available (one could use 5 mL pipet for a final concn of 0.12M too) and the cocn is very close to what we wanted. I suppose, however, that the intent of the problem is to make you think how to make an exact 0.1M solution. Another point to remember is that if you intend to titrate the 2.00 g NaOH will a buret, using 0.1M HCl will require L = moles/M = 0.05/0.1 = 0.5 L or 500 mL. Requiring such a large volume using a 50 mL buret means refilling the buret about 5 times and that increases the reading error immensely. We don't like to do that.)

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry please help!

    Please help. I have no idea how to do these 4 homework problems. 1- How many milliliters of 0.140 M HCl are needed to completely neutralize 42.0mL of 0.106 M Ba(OH)2 solution?
  2. chemistry

    1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution?
  3. Chemistry

    You have an unlimited amount of 12M HCl stock solution. You need to neutralize 2.00 grams of NaOH by slowly adding 0.100M HCl solution.
  4. science

    how to prepare 0.100M HCL solution when laboratory grade concentrated by hydrochloric acid has concentration of 37%.what volume of acid is necessary to prepare 500mL of 0.100M of HCL
  5. chem

    Describe in detail by words how to prepare 200ml of .150M HCl from a 1.00 M HCl stock solution?
  6. Chemistry

    1.What mass of NaOH(s) must be added to 300 mL of HCl 0.25 M in order to completely neutralize this acid?
  7. Chemistry

    Calculate the volume of 2.503 N HNO3 added to 100 mL of HCl in order to prepare 1.1251 N acid solution from the following data: 58.96 mL NaOH will neutralize 2.521g of potassium tetroxalate and 45.57 mL of HCl will neutralize 53.0 …
  8. chemistry

    Solution A:50cm^3 of 1.0mol dm^-3 hydrochloric acid,HCl Solution B:10cm^3 of 2.0mol dm^-3 hydrochloric acid,HCl (a)Calculate the number of moles of hydrochloric acid,HCL in each solution. (b)Solution A and B are mixed together. (i)Calculate …
  9. chemistry

    2. A researcher is often required to prepare solutions in the lab. Typically, a lab provides a concentrated solution. This solution must be diluted to the proper concentration. Hydrochloric acid is a common stock solution that is typically …
  10. chemistry

    A student prepares a solution of hydrochloric acid that is approximately 0.1 M and wanted to determine its precise concentration. A 25.00 mL portion of the HCl solution is transferred to a flask, and after a few drops of indicator …

More Similar Questions