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Chemistry-Common ions

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c=Calculate the OH- conc in a solution containing 6.2x10(-3)M Ba(OH)2 and 1.00x10(-2)M BaCl2?

I thought of using the BaCl2 conc to find the conc of Ba initially, then use that in the ice table for Ba(OH)2, and solve for OH. But i dnot think that's right.
Help? :/

  • Chemistry-Common ions -

    I wonder if this problem expects us to use a Ksp for Ba(OH)2 or not. If not I see no reason to have included the concn of BaCl2. (And note that Ba(OH)2 is quite soluble--I've never even looked for a Ksp for it).(Another note: look in your text and see if Ksp is listed for Ba(OH)2 in Ksp tables. If so we should use it. If not, we don't use it. :-)]

    Assume not a Ksp problem.
    Then Ba(OH)2 --> Ba^2+ + 2OH^-
    If [Ba(OH)2] = 0.0062M then OH^- is twice that.

    If you think it is a Ksp problem then use the BaCl2 as a common ion and solve for OH^-. Repost if you get stuck and explain the problem.

  • Chemistry-Common ions -

    Woooo! the easy way was correct c: Thanks man. But i still kinda don't know why you just doubled it. I thought it would havesomething to do witht he ice table and such since it was in the common ion+buffer chapter :s

    Care explaining or?

  • Chemistry-Common ions -

    You want an ICE chart?
    .........Ba(OH)2 ==> Ba^2+ + 2OH^-

    But I didn't do all of that in my mind. I looked at Ba(OH)2, I see there are 2 OH^- per molecule of Ba(OH)2 and the problem tells me the [Ba(OH)2] = 0.0062M so I know OH^- is twice that.

  • Chemistry-Common ions -

    Wow im an idiot XD thanks.
    And i don't want to be a nuisance, but how would i do the next question?
    0.320M (NH4)2SO4 and 0.492M NH3
    (Still looking for OH- conc)

    Would i find the H+ concentration from the double dissociation of the NH4compound? (i know how to find the oh from there)

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