Question

Define the following: Bronsted-Lowry acid - Lewis acid- Strong acid - (5 points) Problem 6: Consider the following acid base reaction HCI + H20 → H30+ + Cl- a) Is this a strong acid? b) Clearly label the acid, base, conjugate acid and conjugate base. (5 points)

Answer 1

Answer: Yes,
`HCl` is a strong acid.

acid =
`HCl` , conjugate base =
`Cl^-` , base =
`H_2O`, conjugate acid =
`H_3O^+`

Step-by-step explanation:

According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

Yes
`HCl` is a strong acid as it completely dissociates in water to give
`H^+` ions.

`HCl\rightarrow H^++Cl^-`

For the given chemical equation:

`HCl+H_2O\rightarrow H_3O^-+Cl^-`

Here,
`HCl` is loosing a proton, thus it is considered as an acid and after losing a proton, it forms
`Cl^-` which is a conjugate base.

And,
`H_2O` is gaining a proton, thus it is considered as a base and after gaining a proton, it forms
`H_3O^+` which is a conjugate acid.

Thus acid =
`HCl`

conjugate base =
`Cl^-`

base =
`H_2O`

conjugate acid =
`H_3O^+`.