Dissociation constant for a monobasic acid is $10^{-4}$ . What is the $pH$ of the monobasic acid ? (If $\%$ dissociation $= 2\,\%$ )
Dissociation constant for a monobasic acid is $10^{-4}$ . What is the $pH$ of the monobasic acid ? (If $\%$ dissociation $= 2\,\%$ )
- A
$3.2$
- B
$2$
- C
$2.3$
- D
$5$
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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]
A certain amount of $H_2CO_3$ & $HCl$ are dissolved to form $1$ litre solution. At equilibrium it is found that concentration of $H_2CO_3$ & $CO_3^{-\,-}$ are $0.1\,M$ & $0.01\,M$ respectively. Calculate the $pH$ of solution. Given that for $H_2CO_3$ $K_{a_1} =10^{-5}$ & $K_{a_2} =10^{-8}$
A certain amount of $H_2CO_3$ & $HCl$ are dissolved to form $1$ litre solution. At equilibrium it is found that concentration of $H_2CO_3$ & $CO_3^{-\,-}$ are $0.1\,M$ & $0.01\,M$ respectively. Calculate the $pH$ of solution. Given that for $H_2CO_3$ $K_{a_1} =10^{-5}$ & $K_{a_2} =10^{-8}$
Equal volumes of three acid solutions of $pH \,3, 4$ and $5$ are mixed in a vessel. .........$ \times 10^{-4} \,M$ will be the $H^+$ ion concentration in the mixture ?
Equal volumes of three acid solutions of $pH \,3, 4$ and $5$ are mixed in a vessel. .........$ \times 10^{-4} \,M$ will be the $H^+$ ion concentration in the mixture ?
- [AIPMT 2008]
Which among the given acids has lowest $pKa$ value
Which among the given acids has lowest $pKa$ value