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ioda
2 years ago
7

Calculate the percent ionization of benzoic acid at the following concentrations. (a) 0.32 M WebAssign will check your answer fo

r the correct number of significant figures. 1.4 Correct: Your answer is correct. (b) 0.00014 M WebAssign will check your answer for the correct number of significant figures. 48 Correct: Your answer is correct.
Chemistry
1 answer:
seraphim [82]2 years ago
8 0

Answer: a) 1.4 %

b) 48%

Explanation:

C_7H_6O_2\rightarrow H^+C_7H_5O_2^-

 cM                0             0

c-c\alpha    c\alpha      c\alpha  

So dissociation constant will be:

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

a) Given c= 0.32M and K_a=6.3\times 10^{-5}

\alpha = ?

Putting in the values we get:

6.3\times 10^{-5}=\frac{(0.32\times \alpha)^2}{(0.32-0.32\times \alpha)}

(\alpha)=0.014

\%(\alpha)=0.014\times 100=1.4\%

b) Given c= 0.00014 M and K_a=6.3\times 10^{-5}

\alpha = ?

Putting in the values we get:

6.3\times 10^{-5}=\frac{(0.00014\times \alpha)^2}{(0.00014-0.00014\times \alpha)}

(\alpha)=0.48

\%(\alpha)=0.48\times 100=48\%

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