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If the same volume (130-mL) of the buffer were 0.265 M in NH3 and 0.400 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?

I used the henderson-hasselbalch equation to solve this. i set it up as 9=9.24551+log((0.03445-x)/(0.052+x))

0.03445= moles of NH3
0.052= moles of NH4Br

I calculated the grams to be .11 g but it was wrong. Did i set up my H-H equation wrong?

  • Chemistry -

    Assistance needed.

    Please type your subject in the School Subject box. Any other words, including obscure abbreviations, are likely to delay responses from a teacher who knows that subject well.

  • Henderson-Hasselbalch -

    See above for my response.

  • Henderson-Hasselbalch -

    The x is small approximation doesn't work for this problem, so you have to set up an ICE table to solve for the amount of HCl, you can't use the H-H

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