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Delvig [45]
3 years ago
10

Which of the following acids (listed with pKa values) and their conjugate base would form a buffer with a pH of 8.10?

Chemistry
1 answer:
Amiraneli [1.4K]3 years ago
7 0

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 <em>release H⁺</em> and bases are substances that <em>accept H⁺. </em>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.

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Rusting is a chemical reaction between Iron metal [Fe(s)] and oxygen gas [O2(g)] in a slightly acidic environment. Rusting is ac
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Answer:

0.895 mole of Fe₂O₃.

Explanation:

We'll begin by calculating the number of mole in 100 g of Fe. This can be obtained as follow:

Molar mass of Fe = 56 g/mol

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Number of mole of Fe =?

Mole = mass / molar mass

Number of mole of Fe = 100 / 56

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Finally, we shall determine the number of mole of Fe₂O₃ produced by the reaction of 100 g (i.e 1.79 moles) of Fe. This can be obtained as follow:

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From the balanced equation above,

4 moles of Fe reacted to produce 2 moles of Fe₂O₃.

Therefore, 1.79 moles of Fe will react to produce = (1.79 × 2)/4 = 0.895 mole of Fe₂O₃.

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