Which of the following acids (listed with pka values) and their conjugate base would form a buffer with a ph of 8.10?
(a) hc7h5o2, pka = 4.19
(b) hf, pka = 3.46
(c) hclo, pka = 7.54
(d) hcn, pka = 9.31
(e) hclo2, pka = 1.96

(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:

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.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

c) should be the answer.