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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.

Chemistry
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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10 months ago
Balance the equation for ethane C3H6 burning in oxygen to form carbon dioxide and steam. _____C3H6 + ____ O2 ---&gt; CO2 + ____H
aleksandrvk [35]

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2 years ago
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Explanation:

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.

[H^+]=c\alpha = 0.00225M\times 0.08448=0.0001901 M

The pH of the solution ;

pH=-\log[H^+]

=-\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
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