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gtnhenbr [62]
3 years ago
14

consider an exceptionally weak acid, HA, with Ka= 1 x 10-20. you make 0.1M solution of the salt NA. what is the pH.

Chemistry
1 answer:
iogann1982 [59]3 years ago
5 0

Answer:

pH=10.5

Explanation:

Hello,

In this case, the dissociation of the given weak acid is:

HA\rightleftharpoons H^++A^-

Therefore, the law of mass action for it turns out:

Ka=\frac{[H^+][A^-]}{[HA]}

That in terms of the change x due to the reaction extent is:

1x10^{-23}=\frac{x*x}{0.1-x}

Thus, by solving with the quadratic equation or solver, we obtain:

x=31.6x10^{-12}M

Which clearly matches with the hydrogen concentration in the solution, therefore, the pH is:

pH=-log(-31.6x10^{-12})\\pH=10.5

Regards.

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