1. Experiments show that the hydronium ion, H3O, is actually further hydrated so that the proton may have several water molecules associated with it. Why then do we use H3O\', and even more frequently H\', to represent the aqueous proton?
Solution
Actuall H + does not exist in aqueous solutions it is always exist as H 3 O + (aq) and this is correct way of representation. Further, hydronium ion is not a unique species and can pick up additional waters of hydration to form, for example H 5 O 2 + . So, while H 3 O + is more correct than writing H + , it is not prefectly correct. However, we will most often use H + , since more H 2 O is present, as compared with H + when we deal with weak acids for example
HA is a weak acid and dissolved in water now we have
HA (l) + H 2 O (l) <==> H 3 O + (aq) + A - (aq)
dissociation constant K a = [H + ][A - ] / [HA] only
H 3 O + (aq) <==> H + (aq) + H 2 O (l)
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Simple, Complex, and Compound Sentences Exercises.pdf
1- Experiments show that the hydronium ion- H3O- is actually further h.docx
1. 1. Experiments show that the hydronium ion, H3O, is actually further hydrated so that the proton
may have several water molecules associated with it. Why then do we use H3O', and even more
frequently H', to represent the aqueous proton?
Solution
Actuall H +
does not exist in aqueous solutions it is always exist as H 3 O +
(aq) and this is correct
way of representation. Further, hydronium ion is not a unique species and can pick up additional
waters of hydration to form, for example H 5 O 2
+
. So, while H 3 O +
is more correct than writing
H +
, it is not prefectly correct. However, we will most often use H +
, since more H 2 O is
present, as compared with H + when we deal with weak acids for example
HA is a weak acid and dissolved in water now we have
HA (l) + H 2 O (l) <==> H 3 O +
(aq) + A -
(aq)
dissociation constant K a = [H +
][A -
] / [HA] only
H 3 O +
(aq) <==> H +
(aq) + H 2 O (l)
Hope this helped you!
Thank You So Much! Please Rate this answer as you wish.("Thumbs Up")
![1. Experiments show that the hydronium ion, H3O, is actually further hydrated so that the proton
may have several water molecules associated with it. Why then do we use H3O', and even more
frequently H', to represent the aqueous proton?
Solution
Actuall H +
does not exist in aqueous solutions it is always exist as H 3 O +
(aq) and this is correct
way of representation. Further, hydronium ion is not a unique species and can pick up additional
waters of hydration to form, for example H 5 O 2
+
. So, while H 3 O +
is more correct than writing
H +
, it is not prefectly correct. However, we will most often use H +
, since more H 2 O is
present, as compared with H + when we deal with weak acids for example
HA is a weak acid and dissolved in water now we have
HA (l) + H 2 O (l) <==> H 3 O +
(aq) + A -
(aq)
dissociation constant K a = [H +
][A -
] / [HA] only
H 3 O +
(aq) <==> H +
(aq) + H 2 O (l)
Hope this helped you!
Thank You So Much! Please Rate this answer as you wish.("Thumbs Up")](https://image.slidesharecdn.com/1-experimentsshowthatthehydroniumion-h3o-isactuallyfurtherh-230131010801-c35ef578/85/1-Experiments-show-that-the-hydronium-ion-H3O-is-actually-further-h-docx-1-320.jpg)
