13.56 A $$ 2.4 imes 10^{-2} \mathrm{M} $$ solution of benzoic acid is $$ 5.0 \% $$ dissociated. In a C $$ \downarrow 2.4 imes 10^{-3} \mathrm{M} $$ solution, the percentage of dissociation would be meaning a. the same. (b) $$ 5 \% $$ porcent $$

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13.56 A $$ 2.4 	imes 10^{-2} \mathrm{M} $$ solution of benzoic acid is $$ 5.0 \% $$ dissociated. In a C $$ \downarrow 2.4 	imes 10^{-3} \mathrm{M} $$ solution, the percentage of dissociation would be meaning a. the same. (b) $$ >5 \% $$ porcent $$ <5 \% $$ d. zero e. none of these.

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For a weak acid like benzoic acid, the percentage dissociation increases as the concentration of the solution decreases. This is because, according to **Le Chatelier's Principle**, reducing the concentration shifts the equilibrium towards the dissociated form to counteract the change.

Given:
- A 2.4 × 10⁻² M solution of benzoic acid is 5.0% dissociated.
- We're asked about a 2.4 × 10⁻³ M solution.

Since the concentration is decreased by a factor of 10, the percentage dissociation will increase. This is consistent with the formula for percentage dissociation of a weak acid:

$$
\% \text{ dissociation} = \frac{k_a}{C} \times 100\%
$$

Where:
- $$ k_a $$ is the acid dissociation constant.
- $$ C $$ is the concentration of the acid.

As $$ C $$ decreases, $$ \% \text{ dissociation} $$ increases.

**Answer:**  
(b) The percent dissociation is greater than five percent.
The percentage of dissociation increases when the concentration decreases, so in a 2.4 × 10⁻³ M solution, the dissociation is greater than 5%.

13.56 A solution of benzoic acid is dissociated. In a
C solution, the percentage of dissociation would be
meaning a. the same. (b)
porcent
d. zero e. none of these.

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13.56 A solution of benzoic acid is dissociated. In a C solution, the percentage of dissociation would be meaning a. the same. (b) porcent d. zero e. none of these.