Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 1: Exercise 1

Which of the following will occur if $0.1 \mathrm{M}$ solution of a weak acid is diluted to $0.01 \mathrm{M}$ at constant temperature?

When ${\mathrm{CO}}_2$ dissolves in water, the following equilibrium is established: ${\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}\rightleftharpoons {\mathrm{H}}_3{\mathrm{O}}^{+}+{\mathrm{HCO}}_3^{-}$ for which, the equilibrium constant is $3.8\times {10}^{-7}$ and $\mathrm{pH}=6.0$. The ratio of $\left[{\mathrm{HCO}}_3^{-}\right]$ to $\left[{\mathrm{CO}}_2\right]$ would be

The $\mathrm{pOH}$ value of a solution whose hydroxide ion concentration is $6.2\times {10}^{-9} \mathrm{mol} {\mathrm{litre}}^{-1}$ is

A certain buffer solution contains equal concentration of ${\mathrm{X}}^{-}$ and $\mathrm{HX}.$ The ${\mathrm{K}}_{\mathrm{a}}$ for $\mathrm{HX}$ is ${10}^{-8}.$ The $\mathrm{pH}$ of the buffer is

A physician wishes to prepare a buffer solution at $\mathrm{pH}=3.58$ that efficiently resists a change in $\mathrm{pH}$ yet contains only small concentration of the buffering agents. Which one of the following weak acid together with its sodium salt would be best to use?

Which one is not a buffer solution?

Which of the following is a buffer solution with strong acidic nature?

${\mathrm{MnO}}_4^{-}+8{\mathrm{H}}^{+}+5{\mathrm{e}}^{-}⟶{\mathrm{Mn}}^{2+}+4{\mathrm{H}}_2\mathrm{O};$

$\mathrm{E}°=1.51 \mathrm{V}$

${\mathrm{MnO}}_2+4{\mathrm{H}}^{+}+2{\mathrm{e}}^{-}⟶{\mathrm{Mn}}^{2+}+2{\mathrm{H}}_2\mathrm{O}$

$\mathrm{E}°=1.23 \mathrm{V}$

${{\mathrm{E}}^{\circ }}_{{{\mathrm{MnO}}_4}^{-}/{\mathrm{Mno}}_2}$ is