Write examples of weak acids and weak bases and give ionic equilibrium in its aqueous solution.
Write examples of weak acids and weak bases and give ionic equilibrium in its aqueous solution.
| $(A)$ Weak Acids | Ionic Equilibriums |
| $(1)$ Acetic acid $\left(\mathrm{CH}_{3} \mathrm{COOH}\right)$ | $\mathrm{CH}_{3} \mathrm{COOH}_{(\text {aq })}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{H}_{3} \mathrm{O}_{\text {(aq) }}^{+}+\mathrm{CH}_{3} \mathrm{COO}_{\text {(aq) }}^{-}$ |
| $(2)$ Benzoic acid $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)$ | $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}_{(\text {aq })}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{H}_{3} \mathrm{O}_{(\text {aq })}^{+}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}_{(\text {aq })}^{-}$ |
| $(3)$ Hydrocyanic acid $(HCN)$ | $\mathrm{HCN}_{(\text {aq })}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{H}_{3} \mathrm{O}_{\text {(aq) }}^{+}+\mathrm{CN}_{(\text {aq })}^{-}$ |
| $(4)$ Formic acid ($HCOOH$) | $\mathrm{HCOOH}_{(\text {aq })}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{H}_{3} \mathrm{O}_{\text {(aq) }}^{+}+\mathrm{HCOO}_{\text {(aq) }}^{-}$ |
| $(5)$ Hypochlorous acid $(HOCl)$ | $\mathrm{HOCl}_{\text {(aq) }}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{OCl}_{\text {(aq) }}^{-}+\mathrm{H}_{3} \mathrm{O}_{\text {(aq) }}^{+} \text {etc. }$ |
| $(B)$ Weak Bases | Ionic Equilibriums |
| $(1)$ Ammonia $\left(\mathrm{NH}_{3}\right)$ | $\mathrm{NH}_{3(\mathrm{aq})}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{NH}_{4(\mathrm{aq})}^{+}+\mathrm{OH}_{(\mathrm{aq})^{-}}^{-}$ |
| $(2)$ Aniline $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\right)$ | $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2(\mathrm{aq})}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3(\mathrm{aq})}^{+}+\mathrm{OH}_{(\mathrm{aq})}^{-}$ |
| $(3)$ Hydrazine $\left(\mathrm{NH}_{2} \mathrm{NH}_{2}\right)$ | $\mathrm{NH}_{2} \mathrm{NH}_{2(\mathrm{aq})}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{NH}_{2} \mathrm{NH}_{3(\mathrm{aq})}^{+}+\mathrm{OH}_{(\mathrm{aq})}$ |
| $(4)$ Methyl Amine $\left(\mathrm{CH}_{3} \mathrm{NH}_{2}\right)$ | $\mathrm{CH}_{3} \mathrm{NH}_{2(\mathrm{aq})}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square \mathrm{CH}_{3} \mathrm{NH}_{3(\mathrm{aq})}^{+}+\mathrm{OH}_{(\mathrm{aq})}^{-}$ |
| $(5)$ Dimethyl Amine $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}$ | $\left.\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}_{(\mathrm{aq})}+\mathrm{H}_{2} \mathrm{O}_{(l)} \square\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}_{3(\mathrm{aq})}^{+}+\mathrm{OH}_{(\mathrm{aq})}^{-}\right)$etc. |
Similar Questions
Derive the equation of relation between weak base ionization constant ${K_b}$ and its conjugate acid ionization constant ${K_a}$
Derive the equation of relation between weak base ionization constant ${K_b}$ and its conjugate acid ionization constant ${K_a}$
Given
$(i)$ $\begin{gathered}
HCN\left( {aq} \right) + {H_2}O\left( l \right) \rightleftharpoons {H_3}{O^ + }\left( {aq} \right) + C{N^ - }\left( {aq} \right) \hfill \\
{K_a} = 6.2 \times {10^{ - 10}} \hfill \\
\end{gathered} $
$(ii)$ $\begin{gathered}
C{N^ - }\left( {aq} \right) + {H_2}O\left( l \right) \rightleftharpoons HCN\left( {aq} \right) + O{H^ - }\left( {aq} \right) \hfill \\
{K_b} = 1.6 \times {10^{ - 5}} \hfill \\
\end{gathered} $
These equilibria show the following order of the relative base strength
Given
$(i)$ $\begin{gathered}
HCN\left( {aq} \right) + {H_2}O\left( l \right) \rightleftharpoons {H_3}{O^ + }\left( {aq} \right) + C{N^ - }\left( {aq} \right) \hfill \\
{K_a} = 6.2 \times {10^{ - 10}} \hfill \\
\end{gathered} $
$(ii)$ $\begin{gathered}
C{N^ - }\left( {aq} \right) + {H_2}O\left( l \right) \rightleftharpoons HCN\left( {aq} \right) + O{H^ - }\left( {aq} \right) \hfill \\
{K_b} = 1.6 \times {10^{ - 5}} \hfill \\
\end{gathered} $
These equilibria show the following order of the relative base strength
- [AIEEE 2012]
The ionization constant of dimethylamine is $5.4 \times 10^{-4}$. Calculate its degree of ionization in its $0.02$ $M$ solution. What percentage of dimethylamine is ionized if the solution is also $0.1 \,M$ in $NaOH ?$
The ionization constant of dimethylamine is $5.4 \times 10^{-4}$. Calculate its degree of ionization in its $0.02$ $M$ solution. What percentage of dimethylamine is ionized if the solution is also $0.1 \,M$ in $NaOH ?$
At $298$ $K$ temperature, the ${K_b}$ of ${\left( {C{H_3}} \right)_2}NH$ is $5.4 \times {10^{ - 4}}$ $0.25$ $M$ solution.
At $298$ $K$ temperature, the ${K_b}$ of ${\left( {C{H_3}} \right)_2}NH$ is $5.4 \times {10^{ - 4}}$ $0.25$ $M$ solution.
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is