A combination of a weak acid and its conjugate base which is a mix of a weak base and its conjugate acid is so-called a buffer solution or a buffer. Buffer solutions repel a change in pH when small amount of a strong acid or a strong base are additional. Therefore, the best acid to use in the preparation of a buffer with pH=3.3 is HNO₂(Ka = 4.5 * 10 ⁻⁴). The pH of a buffer is contingent on the ration base / acid relatively than on the particular concentration of a precise solution. The precise ratio of the base to the acid for an anticipated pH can be determined from the Ka value and the Henderson HasselBalch equation.
The best acid to use in the preparation of a buffer with pH of 3.3 is Nitrous acid (HNO₂).
Buffer solution is a mixture of weak acid and its conjugate base or weak base and its conjugate acid.
pH of the buffer solution will be calculated by using the Henderson Hasselbalch equation as:
pH = pKa + log[base]/[acid]
From te abive equation it is clear that pH value is directly proportional to the value of pKa. So, for Nitrous acid (HNO₂) value of Ka is 4.5×10⁻⁴ and this will produce a solution of pH 3.3.
Hence best acid is HNO₂.
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