chemistry

posted by .

predict the pH of an aqueous solution that is 0.00378 molar in HBr

  • chemistry -

    HBr is a strong acid; therefore, it ionizes 100%. pH = -log(H^+).

  • chemistry -

    how do i do this one

  • chemistry -

    can we go over this one?

  • chemistry -

    HBr is one of the strong acids. A strong acid ionizes 100%. Therefore, the H^+ concentration is the same as the HBr concentration. You are given the HBr concn, plug that into the equation, and out pops the pH. I shall be happy to check your answer.

  • chemistry -

    so am i just going like this?......
    -log(0.00378)=2.422??

  • chemistry -

    Very good.

  • chemistry -

    yh you are doing grt

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    calculate the pH and the pOH of an aqueous solution that is 0.035 M In HCI and 0.080 M in HBr?
  2. Chemistry

    Predict the products when a chemist mixes an aqueous sodium chloride solution with an aqueous calcium nitrate solution.
  3. ANALYTICAL CHEMISTRY

    3. How many moles of HCl are required to make 15.00 mL of an aqueous 2.500 molar HCl solution?
  4. ANALYTICAL CHEMISTRY

    3. How many moles of HCl are required to make 15.00 mL of an aqueous 2.500 molar HCl solution?
  5. Chemistry

    Calculate the pH and the pOH of an aqueous solution that is 0.025 M in HCl(aq) and 0.075 M in HBr(aq) at 25°C.
  6. Chemistry

    A 100.0mL solution containing aqueous HCl and HBr was titrated with 0.1290M NaOH. The volume of base required to neutralize the acid was 47.56mL. Aqueous AgNO3 was then added to precipitate the Cl- and Br- ions as AgCl and AgBr. The …
  7. 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?
  8. Chemistry

    A 100.0 mL sample of a 0.200 molar aqueous solution of K2CrO4 was added to 100.0 mL of a 0.100 molar aqueous solution of BaCl2. The mixture was stirred and the precipitate was collected, dried carefully, and weighed. How many grams …
  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