MCQ
$\ce{H_2O}$ is a:
- AProton acceptor.
- BRoton donor.
- ✓Both proton donor and proton acceptor.
- DNeither proton donor, nor proton acceptor.
✓
Answer
Correct option: C.
Both proton donor and proton acceptor.
A compound such as water $\ce{(H_2O)}$ has many interesting properties. Water molecules can accept a proton to act as Bronsted $-$ Lowry bases in certain circumstances. The following is an example of $\text{HCl}$ dissolving in water :
$\text{HCl}+\text{H}_2\text{O}(\ell)\rightarrow\text{H}_3\text{O}^+_\text{(aq)}+\text{C}1^-_\text{(aq)}$
The another possibility is water can act like a Bronsted $-$ Lowry acid by donating a proton. Water donates a proton to a proton $-$ accepting amide ion in the presence of ammonia, resulting in the following product:
$\text{H}_2\text{O}\ell{(ℓ)}+\text{NH}^-_2\text{(aq)}\rightarrow\text{OH}^-_{\text{(aq)}}+\text{NH}_3\text{(aq)}$
$\text{HCl}+\text{H}_2\text{O}(\ell)\rightarrow\text{H}_3\text{O}^+_\text{(aq)}+\text{C}1^-_\text{(aq)}$
The another possibility is water can act like a Bronsted $-$ Lowry acid by donating a proton. Water donates a proton to a proton $-$ accepting amide ion in the presence of ammonia, resulting in the following product:
$\text{H}_2\text{O}\ell{(ℓ)}+\text{NH}^-_2\text{(aq)}\rightarrow\text{OH}^-_{\text{(aq)}}+\text{NH}_3\text{(aq)}$
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