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What is the pH of a solution of 0.15 M formic acid?

What is the equilibrium pH of a solution which is initially mixed at 0.200 M in formic acid and 0.00500 M in f?

  • Answer:

    The pKa of formic acid is 3.75. This indicates that the acid does not ionize very much. The F– ion is the conjugate base of the weak acid. Using the Henderon-Hasselblach equation: pH = pKa + log([base]/[acid]) => pH = 3.75 + log([0.00500]/(0.200)[ => pH = 3.75 – 1.60 = 2.15 #6 is the answer!

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The pKa of formic acid is 3.75. This indicates that the acid does not ionize very much. The F– ion is the conjugate base of the weak acid. Using the Henderon-Hasselblach equation: pH = pKa + log([base]/[acid]) => pH = 3.75 + log([0.00500]/(0.200)[ => pH = 3.75 – 1.60 = 2.15 #6 is the answer!

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