Chapter 24.3, Problem 2P

(a)

Interpretation Introduction

Interpretation:

For the given $p{k}_a$ values ADP and phosphoric acid it should be shown that at $pH$7.4 the charge on ATP is -2.8 and -1.8 respectively.

Concept Introduction:

$pH=-\log \left[H^{+}\right]$

The acid dissociation constant of an acid is given by the multiplication of products which is divided by the reactant.

$HA\to H^{+}+A^{-}$

$K_a=\frac{\left[A^{-}\right]\left[H^{+}\right]}{\left[HA\right]}$

(b)

Interpretation Introduction

INTREPRETATION:

For the given $p{k}_a$ values ADP and phosphoric acid it should be shown that at $pH$7.4 the charge on ATP is -2.8 and -1.8 respectively.

CONCEPT INTRODUCTION:

$pH=-\log \left[H^{+}\right]$

The acid dissociation constant of an acid is given by the multiplication of products which is divided by the reactant.

$HA\to H^{+}+A^{-}$

$K_a=\frac{\left[A^{-}\right]\left[H^{+}\right]}{\left[HA\right]}$