Respuesta :
Answer:
(C) HClO, pKa = 7.54
Explanation:
A buffer is a solution that can resist abrupt changes in pH when acids or bases are added. It is formed by two components:
- A weak acid and its conjugate base.
- A weak base and its conjugate acid.
In this case, acid and base are defined according to Bronsted-Löwry theory, which states that acids are substances that release H⁺ and bases are substances that accept H⁺. Therefore, when an acid loses an H⁺ transforms into its conjugated base. For example, HF/F⁻ is a conjugate acid-base pair.
In buffers, when an acid is added, it reacts with the base to diminish its amount:
F⁻ + H⁺ ⇄ HF
Also in buffers, when a base is added, it reacts with the acid to diminish its amount:
HF + OH⁻ = F⁻ + H₂O
The optimum pH range of work of a buffer system (known as buffer range) is between 1 unit less and 1 unit more of pH than its pKa.
So, the buffer formed by HClO/ClO⁻ works optimally in the pH range 6.54-8.54. Since pH = 8.10 is in that interval, this would be the optimal choice.
Answer:
The buffer of pH 8.10 will be formed by the HClO having pKa value of 7.54.
Explanation:
Buffer is defined as the substance that can withstand the changes in the solution due to addition of acid or base. Buffer acts to neutralize the small amounts of acids or base when added.
Buffer is composed of two parts:
A weak acid and its conjugate base and a weak base with its conjugate acid.
According to the Bronsted-Lowry theory, acids are the substances that release [tex]\text {H^{2} }[/tex][tex]\text H^{+}[/tex] , whereas the substances that accept bases.
Similarly, when an acid loses a proton ([tex]\text H^{+}[/tex])[tex]\text {H^{2} }[/tex][tex]\text {H^{+} }[/tex], it is converted into the conjugate base, such that the conjugate acid-base pair of HClO is [tex]\text {H}^{+}/\text{ClO}^{-}[/tex].
The buffer range for a substance is either one unit more or one unit less than the pKa value of the given substance. Thus, to obtain the pH value of 8.10, the acid with pKa value of 7.54 will be selected. The pH range of [tex]\text {H}^{+}/\text{ClO}^{-}[/tex]will have the buffer range between 6.54 and 8.54. Thus, pH of 8.10 will be formed by
Hence, rest of the options are incorrect because the buffer range for given acids will not be close the given value of pH as 8.10.
For Further Reference:
https://brainly.com/question/14353715?referrer=searchResults
