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Concept explainers
Interpretation:
The [H3O+] and pH of a buffer is to be determined consist of 0.55 M HNO2 and 0.75 M KNO2.
Concept introduction:
Buffer solutions are the solutions that resist any change in pH whenever any small amount of acid or alkali are added to it. There are two types of buffer solutions which are as follows:
1. Acidic Buffer- The buffer solutions which are consist of weak acid andits conjugate base with pH less than 7 are known as acidic buffer.
For example: CH3COOH−CH3COONa buffer.
2. Basic Buffer- The buffer solutions which are consist of weak base andits conjugate acid with pH greater than 7 are known as basic buffer. For example: NH4OH−NH4Cl buffer.
The pH of a buffer solution is given by Henderson- Hasselbalch equation which relates the pH with concentration of acid [HA] and concentration of conjugate base [A−] as follows,
pH=pKa+log[A−][HA] (1)
The relation between pKa and Ka is as follows,
pKa=−logKa (2)
The relation between pH and [H3O+] is as follows,
pH=−log[H3O+] (3)
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Chapter 19 Solutions
Chemistry: The Molecular Nature of Matter and Change
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