How do we identify a strong acid in aqueous solution?

Question

How do we identify a strong acid in aqueous solution?

1 Answer

Impact of this question

4423 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-05-18T15:19:51

As you are no doubt aware, this distinction is usually used in the context of $acid/base chemistry$ $"acid/base chemistry"$ .

Explanation:

A strong acid is completely ionized in aqueous solution; viz. for the hydrohalic acids, $H X (X \neq F) :$ $HX(X!=F):$

$H X + H_{2} O (l) ⇌ H_{3} O^{+} + X^{-}$ $HX+H_2O(l) rightleftharpoonsH_3O^+ + X^-$

The strength of an acid depends upon the completion of this equilibrium; i.e. how far the equilibrium to the right. $H I$ $HI$ , $H B r$ $HBr$ , and $H C l$ $HCl$ ARE STRONG ACIDS by this criterion, because dissociation/ionization are almost complete.

On the other hand, weaker acids, incompletely ionize:

$H F (a q) + H_{2} O ⇌ H_{3} O^{+} + F^{-}$ $HF(aq) + H_2O rightleftharpoons H_3O^+ +F^-$

This equilibrium lies to the left as we face it due to (i) the intrinsic strength of the $H - F$ $H-F$ ; and (ii) to the unfavourable entropy effect of the solvated $F^{-}$ $F^-$ conjugate base.

For $H_{2} S O_{4}$ $H_2SO_4$ BOTH conjugate bases are stabilized, and this acts as a diacid in water:

$H_{2} S O_{4} (a q) + H_{2} O (l) \to H S O_{4}^{-} + H_{3} O^{+}$ $H_2SO_4(aq) +H_2O(l) rarr HSO_4^(-) + H_3O^+$

$H S O_{4}^{-} + H_{2} O (l) ⇌ S O_{4}^{2 -} + H_{3} O^{+}$ $HSO_4^(-) + H_2O(l)rightleftharpoonsSO_4^(2-) +H_3O^+$

Science

Math

Humanities

... and beyond

How do we identify a strong acid in aqueous solution?

1 Answer

Explanation:

Related questions

Impact of this question