The pH of a sample of intercellular fluid containing a phosphate buffer with a concentration ratio of H 2 PO 4 − / HPO 4 2 − as 1.1:1 needs to be deduced. Concept Introduction: A buffer is a solution of a weak acid (or base) and it’s salt. The main function of a buffer is to maintain the pH of a solution. The pH of an acidic buffer (HA) is related to the acid dissociation constant Ka via the Henderson-Hasselbalch equation: HA ↔ H + +A − pH = pK a + log [A − ] [ HA] ------ (1) pK a = acid dissociation constant [ A − ] = concentration of the salt/conjugate base [HA] = concentration of the acid

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Chapter 18, Problem 111AE

Interpretation Introduction

Interpretation:

The pH of a sample of intercellular fluid containing a phosphate buffer with a concentration ratio of $H2PO4−/HPO42−$

as 1.1:1 needs to be deduced.

Concept Introduction:

A buffer is a solution of a weak acid (or base) and it’s salt. The main function of a buffer is to maintain the pH of a solution.

The pH of an acidic buffer (HA) is related to the acid dissociation constant Ka via the Henderson-Hasselbalch equation:

$HA↔H++A−pH = pKa + log [A−][HA] ------ (1)pKa = acid dissociation constant[A−] = concentration of the salt/conjugate base[HA] = concentration of the acid$

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