Write the conjugate acids for the following Bronsted bases: $NH_{2}^{-}$,$NH_{3}$ and $HCOO^{-}$.
The conjugate acid of a Bronsted base is formed by adding a proton $(H^{+})$ to the base. The table below lists the conjugate acids for the given Bronsted bases:
| Bronsted base | Conjugate acid |
| $NH_{2}^{-}$ | $NH_{3}$ |
| $NH_{3}$ | $NH_{4}^{+}$ |
| $HCOO^{-}$ | $HCOOH$ |
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Similar Questions
Which among the following is a correct conjugate acid-base pair for the equation stated below?
$HCl + NH_3 \rightleftharpoons NH_4^{+} + Cl^{-}$
$HCl + NH_3 \rightleftharpoons NH_4^{+} + Cl^{-}$
The order of decreasing basic strength of halides is:
Medium
View SolutionChloroplatinic acid is
Medium
View SolutionExplain 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 SolutionRank the following in decreasing order of basic strength:
$A. CH_3 - CH_2 - C \equiv C^-$
$B. CH_3 - CH_2 - S^-$
$C. CH_3 - CH_2 - CO_2^-$
$D. CH_3 - CH_2 - O^-$
$A. CH_3 - CH_2 - C \equiv C^-$
$B. CH_3 - CH_2 - S^-$
$C. CH_3 - CH_2 - CO_2^-$
$D. CH_3 - CH_2 - O^-$
Difficult
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