Answered

As an FDA physiologist, you need 0.700 L of formic acid–formate buffer with a pH of 3.74. (b) How do you prepare this solution from stock solutions of 1.0  M HCOOH and 1.0 M NaOH?



Answer :

 V(HCOOH)=0.4676L solution from stock solutions.

Steps

0.989=xL×1M/(0.7-x)×1M-xL×1M

This V value results from our mathematical calculations:

x=0.2324L=V(KOH)

V(HCOOH)=0.7L−0.2324L=0.4676L

pH buffer: what is it?

Two things affect a buffer's pH: the weak acid's equilibrium constant, Ka; andthe ratio of the weak base, A-, to the weak acid, HA, in the solution. The equilibrium constants of various weak acids varies (Ka). Ka reveals how much of the HA will dissolve into H+ and A- in solution.

The significance of pH buffering

It can keep the pH of the solution largely constant by neutralizing modest amounts of additional acid or base. This is crucial for procedures and/or reactions that call for narrow pH ranges that are stable.

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