You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Percentage Composition

32 g of a sam...

Question

32 g of a sample of $F e S O_{4}$ . $7 H_{2} O$ were dissolved in dilute sulphuric acid and water and its volume was made up to 1 litre. 25 mL of this solution required 20 mL of 0.02 M $K M n O_{4}$ solution for complete oxidation. Calculate the mass % of $F e S O_{4}$ . $7 H_{2} O$ in the sample.

34.75

No worries! We‘ve got your back. Try BYJU‘S free classes today!

69.5

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

89.5

No worries! We‘ve got your back. Try BYJU‘S free classes today!

None of these

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B 69.5
$F e^{+ 2} ⟶ F e^{+ 3}$
$n_{f a c t o r} = 1$
Comparing equivalents of $F e S O_{4} \cdot 7 H_{2} O$ and $K M n O_{4}$
Let molarity of $F e S O_{4} \cdot 7 H_{2} O = M$
$25 \times M \times 1 = 20 \times 0.02 \times 5$
$M = 0.08$ $M o l a r$
No. of moles of $F e S O_{4} \times 7 H_{2} O = 0.08$ $m o l e s$ (Volume $= 1$ Litre)
Mass of $F e S O_{4} \cdot 7 H_{2} O = 0.08 \times 278 = 22.24$ $g m$
$M a s s % = \frac{22.24}{32} \times 100 = 69.5 %$

Suggest Corrections

Similar questions

Q. 32g of a sample of

{F e S O}_{4} . {7 H}_{2} O

where the dissolved in dilute Sulphuric acid and water and it's volume was made up to 1 litre, 25 mL of this solution required 20 mL of 0.02

M K M n O_{4}

solution of complete oxidation. Calculate the weight % of

F e S O_{4} . {7 H}_{2} O

in the sample.

25.0

g of

F e S O_{4} . 7 H_{2} O

was dissolved in water containing dilute

H_{2} S O_{4}

and the volume was made up to

1.0

25

mL of this solution required

20

mL of an

\frac{N}{10} K M n O_{4}

solution for complete oxidation. The percentage of

F e S O_{4} .7 H_{2} O

in the acid solution is:

1.17 g

of an impure sample of oxalic acid was dissolved and made up to

200 m L

with water.

10 m L

of this solution in acid medium required

8.5 m L

of a solution of potassium permanganate containing

3.16 g p e r l i t r e

of oxidation. Calculate the percentage purity of oxalic acid.

12

g of an impure sample of arsenious oxide was dissolved in water containing

7 .5

g of sodium bicarbonate and the resulting solution was diluted to

250

mL.

25

mL of this solution was completely oxidized by

22.4

mL of solution of iodine.

25

mL of this iodine solution reacted with same volume of a solution containing

24.8

g of sodium was completely oxidized by

22.4 m L

of a solution thiosulphate

(N a_{2} S_{2} O_{3} 5 H_{2} O)

in one litre. Calculate the percentage of arsenious oxide in the sample. (Atomic mass of

A s = 75

)

Q. A sample of

F e S O_{4}

and

F e C_{2} O_{4}

was dissolved in dilute sulphuric acid. The complete oxidation of the reaction mixture required 40 mL of N/15

K M n O_{4} .

after the oxidation, the reaction mixture was reduced by Zn and

H_{2} S O_{4} .

On using the same solution of

K M n O_{4}

to oxidize the resulting solution, 25 mL was required. Calculate the ratio of equivalents of Fe in oxalate and Fe(II) sulphate. (Fe: 56)

Join BYJU'S Learning Program

32 g of a sample of FeSO4.7H2O were dissolved in dilute sulphuric acid and water and its volume was made up to 1 litre. 25 mL of this solution required 20 mL of 0.02 M KMnO4 solution for complete oxidation. Calculate the mass % of FeSO4.7H2O in the sample.

The correct option is B 69.5Fe+2⟶Fe+3nfactor=1Comparing equivalents of FeSO4⋅7H2O and KMnO4Let molarity of FeSO4⋅7H2O=M25×M×1=20×0.02×5M=0.08 MolarNo. of moles of FeSO4×7H2O=0.08 moles (Volume =1 Litre)Mass of FeSO4⋅7H2O=0.08×278=22.24 gmMass%=22.2432×100=69.5%

32 g of a sample of $F e S O_{4}$ . $7 H_{2} O$ were dissolved in dilute sulphuric acid and water and its volume was made up to 1 litre. 25 mL of this solution required 20 mL of 0.02 M $K M n O_{4}$ solution for complete oxidation. Calculate the mass % of $F e S O_{4}$ . $7 H_{2} O$ in the sample.