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Marina CMI [18]

3 years ago

10

Calculate the percent dissociation of trimethylacetic acid in a aqueous solution of the stuff. You may find some useful data in

the ALEKS Data resource. Round your answer to significant digits.

1 answer:

LuckyWell [14K]3 years ago

3 0

Answer:

percentage dissociation of trimethylacetic acid in a 0.57M aqueous solution = 0.40%

Explanation:

check attachment below for more information o the answer.

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11 months ago

Balance the equation for ethane C3H6 burning in oxygen to form carbon dioxide and steam. _____C3H6 + ____ O2 ---> CO2 + ____H

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2 years ago

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7 0

3 years ago

Calculate the pH and fraction of dissociation ( α ) for each of the acetic acid ( CH 3 COOH , p K a = 4.756 ) solutions. A 0.002

marysya [2.9K]

Answer:

The degree of dissociation of acetic acid is 0.08448.

The pH of the solution is 3.72.

Explanation:

The $pK_a=4.756$

The value of the dissociation constant = $K_a$

$pK_a=-\log[K_a]$

$K_a=10^{-4.756}=1.754\times 10^{-5}$

Initial concentration of the acetic acid = [HAc] =c = 0.00225

Degree of dissociation = α

$HAc\rightleftharpoons H^++Ac^-$

Initially

c

At equilibrium ;

(c-cα) cα cα

The expression of dissociation constant is given as:

$K_a=\frac{[H^+][Ac^-]}{[HAc]}$

$1.754\times 10^{-5}=\frac{c\times \alpha \times c\times \alpha}{(c-c\alpha)}$

$1.754\times 10^{-5}=\frac{c\alpha ^2}{(1-\alpha)}$

$1.754\times 10^{-5}=\frac{0.00225 \alpha ^2}{(1-\alpha)}$

Solving for α:

α = 0.08448

The degree of dissociation of acetic acid is 0.08448.

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The pH of the solution ;

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$=-\log[0.0001901 M]=3.72$

3 0

3 years ago

PLEASE ANSWER QUICKLY I'M IN A TEST

Natasha_Volkova [10]

D is the correct answer......

hope it help, please thank me if it did.....

4 0

2 years ago

Read 2 more answers