Question

A buffer solution is made using a weak acid, ha, with a pka of 5.43. if the ratio of a– to ha is 0.010, what is the ph of the buffer?

Answer 1

● USING THE "HENDERSON-HASSELBALCH" EQUESTRIAN :-

$= > pH = pKa + \frac{Log[A - ]}{[HA]} \\ \\ = > pH = 5.43 +log(0.010) = 5.43-2 \\ \\ = > pH = 3.43$
________________[ANSWER]

Answer 2

The buffer solution is made using a weak acid, HA, with a pKa of 5.43 and a ratio of the conjugate base (a-) to the weak acid (HA) of 0.010. By using the formula:

pH = pKa + log(a-/HA)

pH = 5.43 + log(0.010)

pH = 5.43 - 2.000

pH = 3.43

The pH of the buffer solution was calculated to be 3.43.

A buffer solution is a solution that can resist changes in pH by rapidly reacting with added acids or bases to restore the initial ratio of its components. This is achieved by combining a weak acid and its conjugate base in the solution. The pH of a buffer is determined by the pKa of the weak acid and the ratio of the conjugate base to the weak acid.

This means that the buffer solution has a pH of 3.43 and can resist changes in pH within a certain range, helping to maintain a relatively constant pH in the solution.

In conclusion, a buffer solution is an important tool in controlling the pH of a solution and helps to maintain a relatively constant pH in the face of changes. Understanding the relationship between the pH of a buffer and its components is crucial for effectively using buffer solutions in various applications.

For more such questions on buffer solutions: https://brainly.in/question/41486102

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