$pH$ of an aqueous solution $H_2CO_3$ is $3.3$. If ${K_{{a_1}}} = {10^{ - 3}}$and ${K_{{a_2}}} = {10^{ - 13}}$ then $[HCO_3^-]$ is

  • A

    $5 \times {10^{ - 4}}\,M$

  • B

    $6 \times {10^{ - 5}}\,M$

  • C

    $3 \times {10^{ - 7}}\,M$

  • D

    $2 \times {10^{ - 3}}\,M$

Similar Questions

What is the $pH$ of $0.001 \,M$ aniline solution? The ionization constant of aniline can be taken from Table . Calculate the degree of ionization of aniline in the solution. Also calculate the ionization constant of the conjugate acid of aniline.

Base $K _{ b }$
Dimethylamine, $\left( CH _{3}\right)_{2} NH$ $5.4 \times 10^{-4}$
Triethylamine, $\left( C _{2} H _{5}\right)_{3} N$ $6.45 \times 10^{-5}$
Ammonia, $NH _{3}$ or $NH _{4} OH$ $1.77 \times 10^{-5}$
Quinine, ( $A$ plant product) $1.10 \times 10^{-6}$
Pyridine, $C _{5} H _{5} N$ $1.77 \times 10^{-9}$
Aniline, $C _{6} H _{5} NH _{2}$ $4.27 \times 10^{-10}$
Urea, $CO \left( NH _{2}\right)_{2}$ $1.3 \times 10^{-14}$

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Calculate $pH$ of $0.02$ $mL$ $ClC{H_2}COOH$. Its ${K_a} = 1.36 \times {10^{ - 3}}$ calculate its $pK_{b}$,

The $ pH$  of $ 0.1$ $M$ acetic acid is $3$, the dissociation constant of acid will be

What is the $pH$ of the resulting solution when equal volumes of $0.1\, M\, NaOH$ and $0.01\, M\, HCl$ are mixed?

  • [NEET 2015]