A solution of a mixture of $\mathrm{KCl}$ and $\mathrm{KOH}$ was neutralized with $120 \mathrm{mL}$ of $0.12 \mathrm{N} \mathrm{HCl}$. After titration, the resultant solution was made acidic with ${\mathrm{HNO}}_3.$ Then, excess of ${\mathrm{AgNO}}_3$ solution was added to precipitate the $\mathrm{AgCl}$ which weighed $3.7 \mathrm{g}$ after drying. Calculate the percentage of $\mathrm{KOH}$in the original mixture. (Give answer up to one decimal point)

Zinc can be determined volumetrically by the precipitation reaction

$3{\mathrm{Zn}}^{2+}+2\left[4{\mathrm{K}}^{+},\mathrm{Fe}(\mathrm{CN}{)}_6^{4+}\right]⟶{\mathrm{K}}_2{\mathrm{Zn}}_3{\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]}_2+6{\mathrm{K}}^{+}$

A sample of zinc ore weighing $1.5432 \mathrm{g}$ was prepared for a reaction and required $34.68 \mathrm{mL}$ of $0.1043 \mathrm{M} {\mathrm{K}}_4\mathrm{Fe}\left(\mathrm{CN}\right)$, for titration. What is the percentage of zinc in the ore?

A chemist is preparing to analyse samples that will contain no more than $0.5 \mathrm{g}$ of uranium. His procedure calls for preparing the uranium as ${\mathrm{U}}^{4+}$ ion and oxidising it by ${{\mathrm{MnO}}_4}^{-}$ in acid solution.

$5{\mathrm{U}}^{4+}+2{\mathrm{MnO}}_4^{-}+6{\mathrm{H}}_2\mathrm{O}\to 5{\mathrm{UO}}_3^{2+}+2{\mathrm{Mn}}^{2+}+4{\mathrm{H}}_3{\mathrm{O}}^{+}$

If he wants to react the total ${\mathrm{U}}^{4+}$ sample with a maximum of $50 \mathrm{mL}$ of ${\mathrm{KMnO}}_4$ solution, concentration he choose is $\mathrm{x} \times {10}^{-2}$

Give the value of $\mathrm{x}$ to the nearest integer value.