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Percentage Composition

40 g of Ba ...

Question

$40$ g of ${B a ({M n O}_{4})}_{2}$ (molecular weight $= 375$ g/mol) sample containing some inert impurities in acidic medium is completely reacted with $125$ mL of $33.6 V$ of $H_{2} O_{2}$ . What is the percentage purity of the sample?

28.12

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70.31

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85

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None of the above

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Solution

The correct option is C $70.31$
Normality of $H_{2} O_{2} = \frac{V o l u m e S t r e n g t h o f H_{2} O_{2}}{5.6}$
$\Rightarrow N_{H_{2} O_{2}} = \frac{33.6}{5.6} = 6$

Equivalents moles of $H_{2} O_{2} = 6 \times 0.125 = 0.750 e q$

Milli Equivalents of $B a (M n O_{4})_{2}$ reacted= Equivalents of $H_{2} O_{2}$ reacted.

Equivalent moles of $B a (M n O_{4})_{2} = \frac{0.75}{10} = 0.075 e q$

Weight of $0.075$ equivalent moles $= 0.075 \times 375 g$

Purity of sample $= \frac{0.075 \times 375}{40} \times 100 = 70.31$ %

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Similar questions

40 g B a (M n O_{4})_{2}

(mol. wt.

= 375

g/mol) sample containing some inert impurities in acidic medium is completely reacted with

125

mL of

33.6 V

H_{2} O_{2}

. What is the percentage purity of the sample?

20

mL of a solution containing

0.2

g of an impure sample of

H_{2} O_{2}

reacts with

0.316

g of

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(acidic medium). Calculate % purity of

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1

g impure sample of

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is treated with

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in acidic medium to produce

H_{3} P O_{4}

and

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requires

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0.2 M

F e S O_{4}

for complete reduction. What is percentage purity of

P_{4} O_{6}

Q. The purity of

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85 %

. Calculate the weight of impure sample of

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P_{2} O_{5} + 3 H_{2} O \to 2 H_{3} P O_{4}

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40 g of Ba(MnO4)2 (molecular weight =375 g/mol) sample containing some inert impurities in acidic medium is completely reacted with 125 mL of 33.6 V of H2O2. What is the percentage purity of the sample?

$40$ g of ${B a ({M n O}_{4})}_{2}$ (molecular weight $= 375$ g/mol) sample containing some inert impurities in acidic medium is completely reacted with $125$ mL of $33.6 V$ of $H_{2} O_{2}$ . What is the percentage purity of the sample?