What is the $ pH$ of $0.01\, M$ glycine solution? For glycine, $K{a_1} = 4.5 \times {10^{ - 3}}$ and $K{a_2} = 1.7 \times {10^{ - 10}}$ at $298 \,K$
What is the $ pH$ of $0.01\, M$ glycine solution? For glycine, $K{a_1} = 4.5 \times {10^{ - 3}}$ and $K{a_2} = 1.7 \times {10^{ - 10}}$ at $298 \,K$
- [AIIMS 2004]
- A
$3$
- B
$10$
- C
$6.1$
- D
$7.2$
Similar Questions
Values of dissociation constant, $K_a$ are given as follows
Acid
$K_a$
$HCN$
$6.2\times 10^{-10}$
$HF$
$7.2\times 10^{-4}$
$HNO_2$
$4.0\times 10^{-4}$
Correct order of increasing base strength of the base $CN^-,F^-$ and $NO_2^-$ will be
Values of dissociation constant, $K_a$ are given as follows
| Acid | $K_a$ |
| $HCN$ | $6.2\times 10^{-10}$ |
| $HF$ | $7.2\times 10^{-4}$ |
| $HNO_2$ | $4.0\times 10^{-4}$ |
Correct order of increasing base strength of the base $CN^-,F^-$ and $NO_2^-$ will be
- [JEE MAIN 2013]
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]
$0.2$ molar solution of formic acid is ionized $3.2\%$. Its ionization constant is
$0.2$ molar solution of formic acid is ionized $3.2\%$. Its ionization constant is
Find $pH$ of $5 \times 10^{-3}\, M$ $H_2CO_3$ solution having $10\%$ dissociation
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The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is
The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is