What is the component concentration ratio, [no2-]/[hno2], of a buffer that has a ph of 3.90? (ka of hno2 = 7.1 * 10-4) ?

Question

Yaritza

Chemistry

8 February, 06:21

What is the component concentration ratio, [no2-]/[hno2], of a buffer that has a ph of 3.90? (ka of hno2 = 7.1 * 10-4) ?

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Answers (1)

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Leon Vaughan · Answer 1

According to Henderson-Hasselbalch Equation,

pH = pKa + log [Nitrate] / [Nitric Acid]

As, Ka of Nitric Acid = 7.1 * 10⁻⁴

So,

pKa = - log [ 7.1 * 10⁻⁴ ]

pKa = 3.148

So, pH = 3.148 + log [Nitrate] / [Nitric Acid]

3.90 = 3.148 + log [Nitrate] / [Nitric Acid]

3.90 - 3.148 = log [Nitrate] / [Nitric Acid]

0.752 = log [Nitrate] / [Nitric Acid]

Taking Antilog on both sides,

[Nitrate] / [Nitric Acid] = 5.64