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3 years ago

In the following reaction: HCO3- (aq) + H2O (aq) → H2CO3 (aq) + OH- (aq)

Chemistry

1 answer:

Basile [38]3 years ago

4 0

Answer:

The correct option is H₂O is an acid and OH⁻ is its conjugate base.

Explanation:

According to the Bronsted-Lowry theory, an acid is a substance capable of yielding a hydrogen ion while a base is a species capable of accepting a hydrogen ion.

A conjugated acid-base pair is a pair of chemical species capable of transforming into each other by exchange of a proton. That is, a conjugated acid is the species that forms after the base accepts a proton. In contrast, a conjugate base is the species that forms after an acid donates its proton.

So, in this case water acts as an acid, yielding a proton to HCO₃⁻, which in turn acts as a base.

The correct option is H₂O is an acid and OH⁻ is its conjugate base.

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Calculate the value of [CH3OH][CO][H2]2 when all concentrations are 2.4. Keep in mind that the reaction may not be at equilibriu

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Explanation:

The given reaction will be as follows.

$CO + 2H_{2} \leftrightharpoons CH_{3}OH$

So, equilibrium constant for this equation will be as follows.

$K_{c} = \frac{[CH_{3}OH]}{[CO][H_{2}]^{2}}$

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$K_{c} = \frac{[CH_{3}OH]}{[CO][H_{2}]^{2}}$

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Thus, we can conclude that equilibrium constant for the given reaction is 0.173.

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3 years ago

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Elena-2011 [213]

Answer:

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