Chemistry

posted by .

If a chemist has a stock solution of HBr that is 10.0 M and would like to make 450.0 mL of 3.0 M HBr, how would he or she do it?

  • Chemistry -

    How many moles do you need in the final solution? That is M x L = x moles
    You want that many mols of the stock solution. You know is it 10 M; therefore, 10 M x ?L = x moles.
    Solve for ?L.

    You may be more comfortable using the dilution formula.
    c1v1 = c2v2
    c= concn
    v = volume

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    A 20.00 ml stock sample of HBr is diluted to 50 mL. If 18.76 ml of 0.1345 M KOH was required to reach the equivalence point, what is the concentration of the stock HBr solution?
  2. chemistry

    A chemist has 12.0 M HBr and would like to use it to make 500.0 mL of 3.5 M HBr. describe how she should do this
  3. Chemistry

    What volume of 14.1M HBr is required to make 250mL of 1.25M HBr solution by dilution with water?
  4. chemistry

    what volume of a 0.272 M solution of HBr is needed for a reaction that requires 49.5 g of HBr?
  5. chemistry

    A chemist makes a “stock” solution of KOH by dissolving 1050.0 grams in enough water to make 1.50 liters of solution. If later on the chemist wants to use this stock solution to make 200.0 mL of 0.10 M KOH, what would the chemist …
  6. chemistry

    Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.180 M pyridine, C5H5N(aq) with 0.180 M HBr(aq): 1)before addition of any HBr 2)after addition of 12.5 ml of HBr: 3)after addition of 16 ml of HBr: 4)after …
  7. Chemistry

    1. Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.240 M pyridine, C5H5N(aq) with 0.240 M HBr(aq): (a) before addition of any HBr (b) after addition of 12.5 mL of HBr (c) after addition of 22.0 mL …
  8. Chemistry

    Let’s assume you have 250 ml of a 1.3M KOH solution and you want to neutralize it with the acid HBr. It takes 350 ml of the HBr solution to do so. What must have been the molarity of the HBr solution?
  9. Chemistry

    Calculate the pH of the the solution that results from titrating 50 mL of 0.6 M NaOCl(aq) with 0.3 M HBr At 0.00 mL of HBr: At 70 mL of HBr: At 100 mL HBr: At 120 mL of HBr
  10. Chemistry

    A 38.5 mL sample of HBr is titrated with 112 mL of 1.05 mol/L KOH. The density of the HBr solution is 1.75 g/mL. Calculate the percentage by mass of the HBr in the sample. How come we don't use density*volume to find the moles of HBr?

More Similar Questions