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determine the pH of a 0.116 M Ba(OH)2 solution at 25 degrees C.

i keep getting 13.06 for this answer, but the answer is 13.37 :S

what i do is i take the negative log of the concentration which is 0.9355 which is pOH.

i know that pH = 14 - pOH
so i get pH = 13.06

where am i going wrong ? :S

thanks for help in advance!

  • Chemistry -

    haha I'm guessing your studying off the old chemistry multiple choice exam for tommorow's chemistry exam at ryerson?

  • Chemistry -

    You assumed barium hydroxide is totally dissociated. The solubility product constant is 5E-3.

  • Chemistry -

    Anya, do you know how to do number 4 on the final chemistry exam. Please tell me.

  • Chemistry -

    i figured it out, i have to multiple the concentration by 2 because of the 2 hydroxides right?

    and yes i do know # 4

    you want to convert 0.0354 mg/mL at 1 atm to mol/L at 0.00036 atm.

    so :

    (0.0354 mg/mL) x ( 0.00036)
    = 1.2744 x 10^-5 mg*CO / mL

    then you just want to convert units)

    1.27 *10^-5 mg*CO/mL is 1.27 * 10 ^-5 g/L

    multiply that by 1 mole CO/ 28 g

    yyou get 4.5 * 10 ^ -7

  • Chemistry -

    Yeah I see what you did. I did the same thing in a slightly different way and got 4.5X10^-5. I see my mistake now

    you have:


    P1=1 C1=0.0354
    P2=0.00036 C2?


    then you cross multiplied and then converted the value 1.27X10^-5 from grams to mols.


    Do you know how to do 6 can you tell me?

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