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Posted by on Sunday, February 27, 2011 at 6:21pm.

Calculate the pH of a solution that results from the mixture of 50.0 mL of 0.15 M HCOOH with 75.0 mL of 0.13 M HCOONa. Now, don't forget these solutions are being mixed and you haven't accounted for that yet in the concentrations! Ka for HCOOH is 1.8 x 10-4.

  • Chemistry - , Sunday, February 27, 2011 at 7:37pm

    moles HCOOH = M x L = ?
    moles HCOONa = M x L = ?
    (HCOOH) = moles/total volume.
    (HCOONa) = moles/total volume.

    Ka = (H^+)(HCOO^-)/(HCOOH)
    Solve for (H^+).
    (HCOO^-) from above.
    (HCOOH) from above.
    Convert (H^+) to pH.
    This is a buffered solution and you can use the Henderson-Hasselbalch equation if you wish. It is a little simpler because you may use moles/V and not actually determine the concns of each (since the volume cancels).

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