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Acetylsalicylic acid (aspirin) behaves a...

Acetylsalicylic acid (aspirin) behaves as an acid according to the equation shown.Calculate `K_b` for the `C_9H_7O_4^-`(aq) ion : `(K_a=3.0xx10^(-4))`
`HC_9H_7O_4(aq)+H_2OhArr H_3O^(+)(aq)+C_9H_7O_4^(-)(aq)`

A

`3.0xx10^(-17)`

B

`3.3xx10^(-11)`

C

`9.0xx10^(-8)`

D

`3.3xx10^(3)`

Text Solution

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The correct Answer is:
b
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The equilibrium equation and K_(a) values for the three acids are given at 25^(@)C : HA(aq)+H_(2)OhArrH_(3)O^(+)(aq)+A^(-)(aq),K_(a)=2xx10^(-5) HB(aq)+H_(2)OhArrH_(3)O^(+)(aq)+B^(-)(aq),K_(a)=4xx10^(-6) HC(aq)+H_(2)OhArrH_(3)O^(+)(aq)+C^(-)(aq),K_(a)=1xx10^(-4) The pH of 0.2M aqueous HA solution is :

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The equilibrium equation and K_(a) values for the three acids are given at 25^(@)C : HA(aq)+H_(2)OhArrH_(3)O^(+)(aq)+A^(-)(aq),K_(a)=2xx10^(-5) HB(aq)+H_(2)OhArrH_(3)O^(+)(aq)+B^(-)(aq),K_(a)=4xx10^(-6) HC(aq)+H_(2)OhArrH_(3)O^(+)(aq)+C^(-)(aq),K_(a)=1xx10^(-4) Which conjugate pair would be best for preparing a buffer witha pH =54? (log 2=0.3).

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