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How to determine if the mixing of two solution would result in buffer solution?

  1. Apr 13, 2007 #1
    1. The problem statement, all variables and given/known data
    Which of the following mixtures would result in buffered solutions whn 1.0 L of each of the two solutions are mixed?

    (i) 0.10 M sodium chloride and 0.10 M sodium nitrite
    (ii) 0.10 M sodium chloride and 0.10 M ammonium chloride
    (iii) 0.10 M hydrochloric acid and 0.10 M ammonia
    (iv) 0.20 M hydrochoric acid and 0.10 M ammonia
    (v) 0.10 M hydrochloric acid and 0.20 M ammonia


    2. Relevant equations

    All I know is that there are 6 methods by which we can buffer solutions:
    (i) weak acid and strong base
    (ii) weak base ans strong acid
    (iii) weak and its salt
    (iv) weak base and its salt
    (v) salt of weak acid and strong acid
    (vi) salt of weak base and strong base



    3. The attempt at a solution

    but when I use the above knowledge, the answer are coming different ... the thing I'm not getting is how the molarity of each of the solutions would have an effect.

    I have the answers for the above parts but I don't know the reasoning .....

    (i) No
    (ii) No
    (iii) No
    (iv) No
    (v) Yes


    Can anyone please please immediately and somehow explain me the reasoning ...... I'll be really thankful ....
     
  2. jcsd
  3. Apr 13, 2007 #2

    Borek

    User Avatar

    Staff: Mentor

    Buffer must contain conjugated pair of acid/base. Preparation methods are a consequence of this.

    Borek
     
    Last edited by a moderator: Aug 13, 2013
  4. Apr 13, 2007 #3
  5. Apr 16, 2007 #4

    Borek

    User Avatar

    Staff: Mentor

    Too late I presume... But to find the answers to your questions you should follow not my links, but information about what the buffer is. Take a look at all solutions defined - IF they contain both acid and conjugated base (especially in comparable quantities) you have a buffer solution.

    Borek
     
    Last edited by a moderator: Aug 13, 2013
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