You have to prepare a pH = 5.00 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH3COOH, CH3COONa, HCN, and NaCN. Which solutions would you use?

Verified step by step guidance

insert step 1> Identify the pKa values of the acids available: HCOOH, CH3COOH, and HCN.

insert step 2> Compare the pKa values to the desired pH of the buffer, which is 5.00.

insert step 3> Choose the acid whose pKa is closest to the desired pH, as this will provide the most effective buffer.

insert step 4> Select the corresponding salt of the chosen acid to pair with it, forming the buffer system.

insert step 5> Use the Henderson-Hasselbalch equation to verify that the chosen acid and its conjugate base can achieve the desired pH.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Buffer Solutions

Buffer solutions are mixtures that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. In this case, a buffer at pH 5.00 can be created using a weak acid and its salt, which helps maintain the desired pH level.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation relates the pH of a buffer solution to the concentration of the acid and its conjugate base. It is expressed as pH = pKa + log([A-]/[HA]), where pKa is the negative logarithm of the acid dissociation constant. This equation is essential for determining the appropriate ratio of acid to base needed to achieve a specific pH.

pKa Values

The pKa value is a measure of the strength of an acid in solution, indicating the pH at which half of the acid is dissociated. For effective buffer preparation, it is important to choose a weak acid with a pKa close to the desired pH. In this scenario, knowing the pKa values of the available acids (HCOOH, CH3COOH, HCN) will help identify which acid-base pair can effectively create a buffer at pH 5.00.

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Textbook Question

You have to prepare a pH = 3.50 buffer, and you have the following 0.10 M solutions available: HCOOH, CH₃COOH, H₃PO₄, HCOONa, CH₃COONa, and NaH₂PO₄. How many milliliters of each solution would you use to make approximately 1 L of the buffer?

Textbook Question

(b) What is the ratio of HCO₃^- to H₂CO₃ in an exhausted marathon runner whose blood pH is 7.1?

Textbook Question

The accompanying graph shows the titration curves for two monoprotic acids. (d) Estimate the pKa of the weak acid.

Textbook Question

You have to prepare a pH = 5.00 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH3COOH, CH3COONa, HCN, and NaCN. How many milliliters of each solution would you use to make approximately 1 L of the buffer?

Textbook Question

You have to prepare a pH = 3.50 buffer, and you have the following 0.10 M solutions available: HCOOH, CH₃COOH, H₃PO₄, HCOONa, CH₃COONa, and NaH₂PO₄. Which solutions would you use?

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