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sammy [17]
4 years ago
13

What is the charge of an oxygen ion? -

Chemistry
2 answers:
olga2289 [7]4 years ago
7 0

The ionic charge of oxygen is -2.

Hope this helps! ;)

cestrela7 [59]4 years ago
5 0

Answer:

-2

Explanation:

Just did it on edge

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A student prepares a aqueous solution of trimethylacetic acid . Calculate the fraction of trimethylacetic acid that is in the di
irinina [24]

The question is incomplete, here is the complete question:

A student prepares a 0.21 mM aqueous solution of trimethylacetic acid. Calculate the fraction of trimethylacetic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 3 significant digits.

<u>Answer:</u> The percent of dissociation of trimethylacetic acid is 19.5 %

<u>Explanation:</u>

We are given:

Concentration of trimethylacetic acid = 0.21 mM  = 0.00021 M    (Conversion factor:  1 mole = 1000 millimoles )

The chemical equation for the dissociation of trimethylacetic acid follows:

                     C_4H_9COOH\rightleftharpoons C_4H_9COO^-+H^+

<u>Initial:</u>                   0.00021

<u>At eqllm:</u>             0.00021-x              x            x

The expression of K_a for above equation follows:

K_a=\frac{[C_4H_9COO^-][H^+]}{[C_4H_9COOH]}

We know that:

K_a\text{ for }C_4H_9COOH=1\times 10^{-5}

Putting values in above expression, we get:

1\times 10^{-5}=\frac{x\times x}{(0.00021-x))}\\\\x=0.000041,-0.000051

Neglecting the negative value of 'x' because concentration cannot be negative.

To calculate the fraction of dissociation, we use the equation:

\text{Percent of dissociation}=\frac{[H^+]}{[C_4H_9COOH]}\times 100

Putting values in above equation, we get:

\text{Percent of dissociation}=\frac{0.000041}{0.00021}\times 100\\\\\text{Percent of dissociation of trimethylacetic acid}=19.5%

Hence, the percent of dissociation of trimethylacetic acid is 19.5 %

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