A mixture of salts was treated to determine the barium content. $\mathrm{A}\, 0.230 \mathrm{~g}$ sample was dissolved and treated with excess potassium chromate. The precipitate of $\mathrm{BaCrO}_4$ was dissolved in dil $\mathrm{HCl}$ to 2 convert $\mathrm{BaCrO}_4$ to $\mathrm{Cr}_2 \mathrm{O}_7^{2-}$ anion. The solution treated with excess sodium iodide and tri lodide produced was titrated with $21 \mathrm{~mL}$ of $0.095 \mathrm{~M}$ sodium thiosulphate. Calculate the $\%$ of $\mathrm{BaCl}_2 . 2 \mathrm{H}_2 \mathrm{O}$ in the sample. [given Molar Mass of $\mathrm{BaCl}_2. 2 \mathrm{H}_2 \mathrm{O}=244$]

JEE CHEMISTRY MCQ: SOME BASIC CONCEPTS OF CHEMISTRY

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A mixture of salts was treated to determine the barium content.

\mathrm{A}\, 0.230 \mathrm{~g}

sample was dissolved and treated with excess potassium chromate. The precipitate of

\mathrm{BaCrO}_4

was dissolved in dil

\mathrm{HCl}

to 2 convert

\mathrm{BaCrO}_4

\mathrm{Cr}_2 \mathrm{O}_7^{2-}

anion. The solution treated with excess sodium iodide and tri lodide produced was titrated with

21 \mathrm{~mL}

0.095 \mathrm{~M}

sodium thiosulphate. Calculate the

\%

\mathrm{BaCl}_2 . 2 \mathrm{H}_2 \mathrm{O}

in the sample. [given Molar Mass of

\mathrm{BaCl}_2. 2 \mathrm{H}_2 \mathrm{O}=244

]

View answer and explanation

Correct option: A

70.5 \%

Option A (70.5 %) is correct because the percentage of BaCl2.2H2O is calculated based on the stoichiometry of the reactions and the titration data.