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Working out the ph of CH3COONa

  1. May 17, 2005 #1
    Hi ppl. I have a question. I'm given the pka of ethanoic acid/ethanoate ions at 4.75 and i have to work out the ph of a 5*10^-2 moldm3 solution of sodium ethanoate. I worked it out by getting the Ka from 10^-4.75 and then saying that the concentration of Ch3COO- in the dissociation of ethanoic acid is also 5*10^-2 moldm3. Then i used the equation for the Ka to get the corresponding concentration of H+ ions in this dissociation and hence the ph, is this method of reasoning correct? Thanks, Joe
  2. jcsd
  3. May 17, 2005 #2


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  4. May 17, 2005 #3


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    The question itself seems to indicate an initial concentration of ethanoate, however, your discussion implies ethanoic acid? Please be more clear...
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