Which of the following species can act as a Bronsted-Lowry acid as well as a Bronsted-Lowry base?
- A$SO_4^{2-}$
- B$HCO_3^{-}$
- C$PO_4^{3-}$
- D$H_2PO_2^{-}$
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Similar Questions
The neutralization of a strong acid by a strong base liberates an amount of energy per mole of $H^{+}$ that:
Medium
View SolutionWhich one of the following compounds will liberate $CO_{2}$ when treated with $NaHCO_{3}$?
Explain the statement: "$NH_3$ acts as both a Lewis base and a Brønsted-Lowry base,whereas $BF_3$ acts only as a Lewis acid but not as a Brønsted-Lowry acid."
Difficult
View SolutionMatch the following:
List-$I$ (Acid) List-$II$ ($K_a$ - Ionization Constant) $A$. $HCN$ $I$. $6.8 \times 10^{-4}$ $B$. $H_2C_2O_4$ $II$. $8.9 \times 10^{-8}$ $C$. $H_2S$ $III$. $4.9 \times 10^{-10}$ $D$. Niacin $IV$. $5.6 \times 10^{-2}$ $V$. $1.5 \times 10^{-5}$
The correct match is:
| List-$I$ (Acid) | List-$II$ ($K_a$ - Ionization Constant) |
| $A$. $HCN$ | $I$. $6.8 \times 10^{-4}$ |
| $B$. $H_2C_2O_4$ | $II$. $8.9 \times 10^{-8}$ |
| $C$. $H_2S$ | $III$. $4.9 \times 10^{-10}$ |
| $D$. Niacin | $IV$. $5.6 \times 10^{-2}$ |
| $V$. $1.5 \times 10^{-5}$ |
The correct match is:
The conjugate base of $NH_{3}$ is
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