help with buffers please?

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What is the pH of a buffer that consists of 0.58 M HCOOH and 0.71 M HCOONa? pKa of formic acid = 3.74.

2006-10-24 07:50:57 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry

You can use the Henderson-Hasselbalch formula:

pH = pKa + log([HCOONa]/[HCOOH]

pH = 3.74 + log(0.71/0.58)

pH = 3.74 + 0.09, pH = 3.83

2006-10-24 08:05:29 · answer #1 · answered by Dimos F 4 · 0⤊ 0⤋

A buffer is defined by the henderson-hasselbach equation:
pH = pKa + log( [base] / [acid])
pH = 3.74 + log (0.71/0.58)
pH = 3.74 + 0.088
pH = 3.83

2006-10-24 15:55:06 · answer #2 · answered by davisoldham 5 · 0⤊ 0⤋