Chemistry: The percentage deprotonation of a 0.115 M solution of benzoic acid (a weak, monoprotic acid) is 2.1%. What is the pH of the solution

The percentage deprotonation of a 0.115 M solution - id01155164547, markitakimbrough69

Ответ:

lesl26

19.01.2022

Chemistry

The pH value of the solution is : 2.6

Given data:

percentage deprotonation = 2.1%

concentration of solution ( c ) = 0.115 M

Determine the pH of the solution

Applying dissociation constant ; K $_{a}$ = $\frac{(c\alpha)^{2} }{c-c\alpha }$ ( HA ---> H⁺A⁻ )

∝ = $\frac{2.1}{100}$ = 0.021

[ H⁺ ] = c * ∝ = 0.115 * 0.021 = 0.0024

Given that

pH = -log [ H⁺ ]

pH = - log [ 0.0024 ]

∴ pH of the solution = 2.6

Hence we can conclude that the pH of the solution is 2.6

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Ответ:

zb868469

19.01.2022

Chemistry

pH of the solution is 2.6

Explanation:

$HA\rightarrow H^+A^-$

cM 0 0

$c-c\alpha$ $c\alpha$ $c\alpha$

So dissociation constant will be:

$K_a=\frac{(c\alpha)^{2}}{c-c\alpha}$

Give c= 0.115 M and $\alpha$ = $\frac{2.1}{100}=0.021$

$(\alpha)=0.030$

$[H^+]=c\times \alpha$

$[H^+]=0.115\times 0.021=0.0024$

Also pH=-log[H^+]

pH=-log[0.0024]=2.6

Thus pH of the solution is 2.6

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Ответ:

deedee2094

28.08.2022

Chemistry

cutie :

cowboy

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The percentage deprotonation of a 0.115 M solution of benzoic acid (a weak, monoprotic acid) is 2.1%. What is the pH of the solution

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