Advertisements
Advertisements
Question
Conjugate base for Bronsted acids H2O and HF are ___________.
Options
OH– and H2FH+, respectively
H3O+ and F–, respectively
OH– and F–, respectively
H3O+ and H2F+, respectively
Advertisements
Solution
Conjugate base for Bronsted acids H2O and HF are OH– and F–, respectively.
Explanation:
\[\ce{\underset{acid 1}{H2O} + \underset{base 1}{H2O} ⇌ \underset{acid 2}{H3O^+} + \underset{base 2}{OH^-}}\]
\[\ce{\underset{acid 1}{HF} + \underset{base 1}{H2O} ⇌ \underset{acid 2}{H3O^+} + \underset{base 2}{F^-}}\]
∴ Conjugate bases are OH− and F− respectively.
APPEARS IN
RELATED QUESTIONS
The theory which explain amphoteric nature of water is ______.
Classify the following species into Lewis acids and Lewis bases.
| Cl- | |
| `"NH"_4^+` | |
| BCl3 | |
| NH3 |
In which oxidation state, group 15 elements act as Lewis base?
Which of the following fluro compounds is most likely to behave as a Lewis base?
Which of these is not likely to act as Lewis base?
Identify the conjugate acid-base pair for the following reaction in an aqueous solution.
\[\ce{NH^+_4 + CO^{2-}_3 ⇌ NH3 + HCO^-_3}\]
Name one amphoteric solvent.
Identify the conjugate acid - base pair in the following reaction.
\[\ce{H2O + HCl -> H3O+ + Cl-}\]
Which of the following species is amphoteric in nature?
The species which will behave both as conjugate acid and conjugate base is ______.
