The [ H 3 O + ] and the pH of a buffer is to be determined which is consist of 0.95 M HBrO and 0.68 M KBrO . 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: CH 3 COOH − CH 3 COONa 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: NH 4 OH − NH 4 Cl 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 = p K a + log [ A − ] [ HA ] (1) The relation between pH and [ H 3 O + ] is as follows, pH = − log [ H 3 O + ] (2)

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Chapter 19, Problem 19.17P

Interpretation Introduction

Interpretation:

The $[H3O+]$ and the $pH$ of a buffer is to be determined which is consist of $0.95 M HBrO$ and $0.68 M KBrO$ .

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 $pH$ and $[H3O+]$ is as follows,

$pH=−log[H3O+]$ (2)

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