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miskamm [114]
3 years ago
6

Calculate [H3O+] and [OH−] for each of the following solutions at 25 ∘C given the pH. pH= 2.89

Chemistry
1 answer:
dimaraw [331]3 years ago
6 0

Answer: The value of [H_{3}O^{+}] is 0.0012 M and [OH^{-}] is 1.02 \times 10^{-14}.

Explanation:

pH is the negative logarithm of concentration of hydrogen ion.

It is given that pH is 2.89. So, the value of concentration of hydrogen ions is calculated as follows.

pH = - log [H^{+}]\\2.89 = - log [H^{+}]\\conc. H^{+} = 0.0012 M

The relation between pH and pOH value is as follows.

pH + pOH = 14

0.0012 + pOH = 14

pOH = 14 - 0.0012 = 13.99

Now, pOH is the negative logarithm of concentration of hydroxide ions.

Hence, [OH^{-}] is calculated as follows.

pOH = - log [OH^{-}]\\13.99 = - log [OH^{-}]\\conc. OH^{-} = 1.02 \times 10^{-14} M

Thus, we can conclude that the value of [H_{3}O^{+}] is 0.0012 M and [OH^{-}] is 1.02 \times 10^{-14}.

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Putting values in above equation, we get:

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