As an FDA physiologist, you need 0.700 L of formic acid–formate buffer with a pH of 3.74. (a) What is the required buffer-component concentration ratio?

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23-08-2022
Chemistry

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As an FDA physiologist, you need 0.700 L of formic acid–formate buffer with a pH of 3.74. (a) What is the required buffer-component concentration ratio?

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Tutorconsortium328 Tutorconsortium328 · Answer 1 · 2022-08-29T11:10:37-04:00

The required buffer-component concentration ratio is [tex]\frac{A}{HA} =0.989[/tex]

Steps

To determine the acid base ratio, we can use the Henderson-Hasselbatch equation: Ka(HCOOH) = [tex]1.8$\times10{^{-4}}$[/tex]

[tex]PH= PKa+log \frac{A}{HA}[/tex]

3.74=[tex]1.8$\times10{^{-4}}$+logA/HA[/tex]

[tex]\frac{A}{HA} =0.989[/tex]

The required buffer-component concentration ratio is [tex]\frac{A}{HA} =0.989[/tex]

Describe pH buffer.

The equilibrium constant Ka of the weak acid and the ratio of weak base (A-) to weak acid (HA) in solution are the two variables that determine the pH of a buffer. 1) The equilibrium constants of different weak acids vary (Ka). Ka tells us how much of the HA in the solution will be dissolved into H+ and A-.

What makes pH buffering crucial?

Small additions of acid or base can be neutralized by it, keeping the pH of the solution largely constant. For procedures and/or reactions that call for particular and stable pH ranges, this is significant.

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