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osimsDDS

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SO/NOR-CAL
  1. Pre-Dental
    assuming this is a weak monoprotic acid, the concentration of H+ in the solution is going to be equal to the concentration of the conjugate base. Therefore, it should be 10^-2.7 which is close to 2 * 10^-3.
    I would pick B.

    you mean C harry, 2x10^-3 is answer choice C...

    I actually agree with you, because the dissociation assuming its a monoprotic acid like you said will make up H+ and the conjugate base, therefore the H+ concentration should equal the conjugate base concentration...
     

    harrygt

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    1. Pre-Dental
      you mean C harry, 2x10^-3 is answer choice C...

      I actually agree with you, because the dissociation assuming its a monoprotic acid like you said will make up H+ and the conjugate base, therefore the H+ concentration should equal the conjugate base concentration...

      Yeah, I meant choice C. Sorry about that. It was just a typo. Danny, you mean the answer is not C?
       

      HoangDDS

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      1. Pre-Dental
        you mean C harry, 2x10^-3 is answer choice C...

        I actually agree with you, because the dissociation assuming its a monoprotic acid like you said will make up H+ and the conjugate base, therefore the H+ concentration should equal the conjugate base concentration...

        if the PH of the weak acid is 2.7, then the [H+] = 2 x 10^-3M , but I dont understand why that would equal the conjugate base?
         
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        harrygt

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          Harry,would tell me so when do we use Henderson-Hasselbach Equation.I'm very confuse about this subject?

          We could have used Henderson-... if we had the pka of the acid.

          PH - pka = log A-/HA

          This is really simple. if 1 mole of 10 moles of HA dissociates, you will have 1 mole of H+ and 1 mol of A-. concentration of H+ and A- will be the same.
           
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