(Solved): Determine the concentration of C6H5NH3+in a buffer solution by constructing an ICE table, ...

Determine the concentration of ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_3{}^{+}$in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_3{}^{+}$. The $\mathrm{Kb}$ for ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_2$ is $3.8\times 10^{?10}$. Complete Parts $1?3$ before submitting your answer. A buffer solution contains dissolved ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_2$ and ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_3\mathrm{Cl}$. The initial concentration of ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_2$ is $0.50\mathrm{M}$. The $\mathrm{pH}$ at equilibrium of the buffer is 4.20 . Let $x$ represent the original concentration of ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_3{}^{+}$in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.