Question

Why are hydrogen ions NEVER found in an aqueous solution?


HCN(aq) + SO4-2(aq) HSO4-(aq) + CN -(aq)

What is the Bronsted - Lowry acid in this equation?
What is the Bronsted - Lowry base in this equation?
What is the conjugate acid in this equation?
What is the conjugate base in this equation?

Answer 1

Answer on the question #50447, Chemistry, Other

Question:

Why hydrogen ions are NEVER found in an aqueous solution?

HCN(aq) + SO4-2(aq) HSO4-(aq) + CN -(aq)

What is the Bronsted - Lowry acid in this equation?

What is the Bronsted - Lowry base in this equation?

What is the conjugate acid in this equation?

What is the conjugate base in this equation?

Answer:

1) The hydrogen ions are never found in the solutions because they always exist in the H3O+ form. This originates from the true water autoionisation reaction:

$$H _ {2} O + H _ {2} O \rightleftharpoons H _ {3} O ^ {+} + O H ^ {-}$$

2)

$$H C N + S O _ {4 (a q)} ^ {2 -} \rightleftharpoons H S O _ {4 (a q)} ^ {-} + C N _ {(a q)} ^ {-}$$

the Bronsted - Lowry acid is the HCN, because it donates hydrogen ion;

the Bronsted - Lowry base is $SO_{4(aq)}^{2-}$, because it accepts the hydrogen ion;

the conjugate acid is the $HSO_{4(aq)}^{-}$, the conjugate base $-CN_{(aq)}^{-}$.

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