In the equation $H C l (g) + H_{2} O (l) \to H_{3} O^{+} (a q) + C l^{-} (a q)$ $HCl(g) + H_2O(l) -> H_3O^+(aq) + Cl^(-)(aq)$ , which species is a Bronsted-Lowry acid?

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In the equation $H C l (g) + H_{2} O (l) \to H_{3} O^{+} (a q) + C l^{-} (a q)$ $HCl(g) + H_2O(l) -> H_3O^+(aq) + Cl^(-)(aq)$ , which species is a Bronsted-Lowry acid?

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Answer 1 · 2016-01-01T23:44:04

Hydrochloric acid, $HCl$ $"HCl"$ .

Explanation:

As you know, a Bronsted - Lowry acid is a proton donor, which means that you can identify a Bronsted - Lowry acid in a reaction by looking at which chemical species lost a proton.

A proton is simply a hydrogen ion, $H^{+}$ $"H"^(+)$ , so the species that has one less proton on the products' side than it does on the ractants' side will be the Bronsted - Lowry acid.

In your case, you have

$H {Cl}_{(aq]} + H_{2} O_{(l]} \to H_{3} O_{(aq]}^{+} + {Cl}_{(aq]}^{-}$ $color(red)("H")"Cl"_text((aq]) + "H"_2"O"_text((l]) -> "H"_3"O"_text((aq])^(color(red)(+)) + "Cl"_text((aq])^(-)$

Notice that hydrochloric acid, $HCl$ $"HCl"$ , starts with a proton that ends up on a water molecule, which acts as a Bronsted - Lowry base, and forms hydronium ions, $H_{3} O^{+}$ $"H"_3"O"^(+)$ .

The remaining chloride anion, ${Cl}^{-}$ $"Cl"^(-)$ , is called the acid's conjugate base because it can theoretically reform the acid by aaccepting a proton.

Since hydrochloric acid donated a proton, it acted as a Bronsted - Lowry acid.

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In the equation $H C l (g) + H_{2} O (l) \to H_{3} O^{+} (a q) + C l^{-} (a q)$ $HCl(g) + H_2O(l) -> H_3O^+(aq) + Cl^(-)(aq)$ , which species is a Bronsted-Lowry acid?

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Explanation:

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In the equation HCl(g)+H2O(l)→H3O+(aq)+Cl−(aq)HCl(g) + H_2O(l) -> H_3O^+(aq) + Cl^(-)(aq), which species is a Bronsted-Lowry acid?

1 Answer

Explanation:

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In the equation $H C l (g) + H_{2} O (l) \to H_{3} O^{+} (a q) + C l^{-} (a q)$ $HCl(g) + H_2O(l) -> H_3O^+(aq) + Cl^(-)(aq)$ , which species is a Bronsted-Lowry acid?