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krek1111 [17]
3 years ago
8

What is the ph of a buffer prepared by adding 0.809 mol of the weak acid ha to 0.608 mol of naa in 2.00 l of solution? The disso

ciation constant ka of ha is 5.66×10−7.
Chemistry
1 answer:
Anarel [89]3 years ago
5 0

The pH of the buffer is 6.1236.

Explanation:

The strength of any acid solution can be obtained by determining their pH. Even the buffer solution strength of the weak acid can be determined using pH. As the dissociation constant is given, we can determine the pKa value as the negative log of dissociation constant value.

pKa=-log[H] = - log [ 5.66 * 10^{-7}]\\ \\pka = 7 - log (5.66)=7-0.753=6.247\\\\pka = 6.247

The pH of the buffer can be known as

pH = pK_{a} + log[\frac{[A-]}{[HA]}}]

The concentration of [A^{-}] = Moles of [A]/Total volume = 0.608/2 = 0.304 M\\

Similarly, the concentration of [HA] = \frac{Moles of HA}{Total volume} = \frac{0.809}{2} = 0.404

Then the pH of the buffer will be

pH = 6.247 + log [ 0.304/0.404]

pH = 6.247 + log 0.304 - log 0.404=6.247-0.517+0.3936=6.1236

So, the pH of the buffer is 6.1236.

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<em>Statements describe polyatomic ions</em>

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<h3><em>Further explanation</em></h3>

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So the correct answer is:

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<h3><em>Learn more</em></h3>

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<h3><em>Answer details </em></h3>

Grade: Senior High School

Subject: Chemistry

Chapter: Atomic Structure

Keywords: ion, polyatomic, ionic bonds, atom

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