MyQuestionIcon

1

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

Stoichiometric Calculations

25.0 g of F...

Question

$25.0$ 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 $1.0$ L. $25.0$ mL of this solution required $20$ mL of $\frac{N}{10} K M n O_{4}$ solution for complete oxidation. The percentage of $F e S O_{4} .7 H_{2} O$ in the acidic solution is :

A

78 %

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

B

98 %

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

C

89 %

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

D

79 %

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

Open in App

Solution

The correct option is C $89 %$
Mili equivalents of $F e S O_{4} .7 H_{2} O$ in $25$ ml $=$ Milli equivalents of $K M n O_{4}$ used $= 2$ milli equivalents

Milli equivalents of $F e S O_{4} .7 H_{2} O$ in $1000$ ml $= 80$ milli equivalents.

Mass of $F e S O_{4} .7 H_{2} O$ in solution = $\frac{80}{1} \times 278 \times \frac{1}{1000} = 22.24$ g

$%$ of $F e S O_{4} .7 H_{2} O = \frac{22.24}{25} \times 100 = 88.89 = 89 %$

Suggest Corrections

thumbs-up

0

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

Q. 0.2828 g of iron wire was dissolved in excess of dilute

H_{2} S O_{4}

and the solution was made upto 100 ml. 20 ml of this solution required 30 ml. of

\frac{N}{30} K_{2} C r_{2} O_{7}

solution for oxidation. Calculate % purity of iron in the wire:

Q. 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

Q. A mixture of

H_{2} S O_{4}

H_{2} C_{2} O_{4}

(oxalic acid) and some inert impurity weighing

3.185 g

was dissolved in water and the solution made up to

1 L

10 m L

of this solution required

3 m L

0.1 N N a O H

for complete neutralization. In another expriment

100 m L

of the same solution in hot condition required

4 m L

0.02 M K M n O_{4}

solution for complete reaction. The weight percentage of

H_{2} S O_{4}

in the mixture was:

1.17 g

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

200 m L

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.

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Stoichiometric Calculations

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Stoichiometric Calculations

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon