Q10P When is a weak acid weak and whe... [FREE SOLUTION]

Chapter 9: Q10P (page 208)

When is a weak acid weak and when is a weak acid strong? Show that the weak acid $99 %$ dissociatedrole="math" localid="1654854665468" $F = (0.0102) K_{a}$ will be 92%dissociated when dissolved in water if the formal concentration is one-tenth $(F = Ka / 10)$ of Show that the fraction of dissociation is 27%when $F = 10 Ka$ . At what formal concentration will the acid be 99%dissociatedCompare your answer with the left -hand curve in Figure 9-2

Expert verified

The formal concentration at which the acid would be 99%dissociated, $F = (0.0102) K_{a}$

It is the process of breaking up of a compound into simper constituents that are able to recombining under other conditions.

$HA \overset{}{鈬�} H^{+} + A^{-} [HA] = F - X [H^{+}] + [A^{-}] = XH$

The constant of disassociation is written as:

$K_{a} = \frac{x^{2}}{F - x}$

The fraction of disassociation is 27% where $F = 10 K_{a}$ , then,

$K_{a} = \frac{x^{2}}{K_{a} / 10 - x} x = 0.092 K_{a} a = X / F = 0.092 K_{a} / 0.100 K_{a} = 92 %$

By determining forma concentration at which the acid would be 99% dissociated:

$x = 0.99 F K_{a} = \frac{x^{2}}{F - x} K_{a} = \frac{{(0.99 F)}^{2}}{F - (0.99 F)} F = (0.0102) K_{a}$

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