A $0.1\,N $ solution of an acid at room temperature has a degree of ionisation $ 0.1$ . The concentration of $O{H^ - }$ would be
A $0.1\,N $ solution of an acid at room temperature has a degree of ionisation $ 0.1$ . The concentration of $O{H^ - }$ would be
- A
${10^{ - 12}}\,M$
- B
${10^{ - 11}}\,M$
- C
${10^{ - 9}}\,M$
- D
${10^{ - 2}}\,M$
Similar Questions
Dimethyl amine ${\left( {C{H_3}} \right)_2}NH$ is weak base and its ionization constant $ 5.4 \times {10^{ - 5}}$. Calculate $\left[ {O{H^ - }} \right],\left[ {{H_3}O} \right]$, $pOH$ and $pH$ of its $0.2$ $M$ solution at equilibrium.
Dimethyl amine ${\left( {C{H_3}} \right)_2}NH$ is weak base and its ionization constant $ 5.4 \times {10^{ - 5}}$. Calculate $\left[ {O{H^ - }} \right],\left[ {{H_3}O} \right]$, $pOH$ and $pH$ of its $0.2$ $M$ solution at equilibrium.
Which of the following will occur if a $0.1 \,M$ solution of a weak acid is diluted to $0.01\,M$ at constant temperature
Which of the following will occur if a $0.1 \,M$ solution of a weak acid is diluted to $0.01\,M$ at constant temperature
The concentration of $[{H^ + }]$ and concentration of $[O{H^ - }]$ of a $ 0.1$ aqueous solution of $2\%$ ionised weak acid is [Ionic product of water $ = 1 \times {10^{ - 14}}]$
The concentration of $[{H^ + }]$ and concentration of $[O{H^ - }]$ of a $ 0.1$ aqueous solution of $2\%$ ionised weak acid is [Ionic product of water $ = 1 \times {10^{ - 14}}]$
- [AIPMT 1999]
If degree of ionisation is $0.01$ of decimolar solution of weak acid $HA$ then $pKa$ of acid is
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The $pH$ of $ 0.1 \,M$ solution of a weak monoprotic acid $1\%$ ionized is
The $pH$ of $ 0.1 \,M$ solution of a weak monoprotic acid $1\%$ ionized is