$0.5 \mathrm{~g}$ mixture of oxalic acid $\left(\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4\right)$ and some sodium oxalate $\left(\mathrm{Na}_2 \mathrm{C}_2 \mathrm{O}_4\right)$ with some impurities requires $40 \mathrm{~ml}$ of $0.1 \mathrm{~M} \mathrm{~NaOH}$ for complete neutralization and $6 \mathrm{~ml}$ of $0.2 \mathrm{~M} \, \mathrm{KMnO}_4$ for complete oxidation. Calculate the $\%$ of $\mathrm{Na}_2 \mathrm{C}_2 \mathrm{O}_4$ in the mixture.

NEET UG CHEMISTRY MCQ: PRACTICAL CHEMISTRY

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Analyzing +4 | -1

0.5 \mathrm{~g}

mixture of oxalic acid

\left(\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4\right)

and some sodium oxalate

\left(\mathrm{Na}_2 \mathrm{C}_2 \mathrm{O}_4\right)

with some impurities requires

40 \mathrm{~ml}

0.1 \mathrm{~M} \mathrm{~NaOH}

for complete neutralization and

6 \mathrm{~ml}

0.2 \mathrm{~M} \, \mathrm{KMnO}_4

for complete oxidation. Calculate the

\%

\mathrm{Na}_2 \mathrm{C}_2 \mathrm{O}_4

in the mixture.

View answer and explanation

Correct option: B

26.8 \%

Option B (26.8 %) is correct because it involves calculating the amount of oxalic acid and sodium oxalate in the mixture using the given neutralization and oxidation data, then finding the percentage of sodium oxalate.

More Questions from PRACTICAL CHEMISTRY

Practice All Chapter MCQs →

A pale green crystalline inorganic salt (A) dissolves freely in water. It gives a brown precipitate on addition of aqueous

\mathrm{NaOH}.

The solution of (A) also gives a black precipitate on bubbling

\mathrm{H}_2 \mathrm{S}

in alkaline medium. An aqueous solution of the (A) decolorizes the pink colour of the permanganate solution. The metal in the salt solution is

100 \mathrm{~ml}

\mathrm{NaHC}_2 \mathrm{O}_4

required

50 \mathrm{~ml}

0.1 \mathrm{~M} \, \mathrm{KMnO}_4

solution in acidic medium. Volume of

0.1 \mathrm{~M} \mathrm{~NaOH}

required by

100 \mathrm{~ml}

\mathrm{NaHC}_2 \mathrm{O}_4

is The ion that cannot be precipitated by both

{HCl}

and

{H}_2 {S}

is The rapid change of pH near the stoichiometric point of an acid-base titration in the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugated acid

(HIn)

and the base

(In)

forms of the indicator by the expression. On heating colourless solid

A,

gas

B

(liquid at room temp.) and gas

C

are formed.

A

is decomposed by

\mathrm{NaOH}

on heating to form gas

D

giving white fumes with

\mathrm{HCl}.

Gas

{C}

occupies

800 \mathrm{~ml} / \mathrm{g}

at N.T.P. Hence

A

is Standard

HCl

solution is titrated to a pink phenolphthalein endpoint by adding a

\mathrm{NaOH}

solution while stirring. If a solution becomes pink throughout but loses its color upon standing for a short time, what should be done to restore the color?