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kari74 [83]
3 years ago
5

Helppppppppppppppppppppppppp

Chemistry
1 answer:
sergey [27]3 years ago
8 0

Answer:

lose 1 2+

Explanation:

I honestly don't know

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Calculate [H3O+] and [OH−] for each of the following solutions at 25 ∘C given the pH.<br> pH= 2.89
dimaraw [331]

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.

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

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pH + pOH = 14

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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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