${K_a} = 1.4 \times {10^{ - 5}}$ of propanoic acid. Calculate its $pH$ of $0.1$ $M$ solution.
${K_a} = 1.4 \times {10^{ - 5}}$ of propanoic acid. Calculate its $pH$ of $0.1$ $M$ solution.
$\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.2 \times 10^{-3}, \mathrm{pH}=2.92$
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Write examples of weak acids and weak bases and give ionic equilibrium in its aqueous solution.
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$0.01$ moles of a weak acid $HA \left( K _{ a }=2.0 \times 10^{-6}\right)$ is dissolved in $1.0\, L$ of $0.1\, M\, HCl$ solution. The degree of dissociation of $HA$ is ............. $\times 10^{-5}$
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[Neglect volume change on adding $HA$. Assume degree of dissociation $<< 1]$
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(Round off to the Nearest Integer).
[Neglect volume change on adding $HA$. Assume degree of dissociation $<< 1]$
- [JEE MAIN 2021]
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