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

Byju's Answer

Standard XII

Chemistry

Hydrochloric Acid

A sample 5.6 ...

Question

A sample (5.6 g) containing iron is completely dissolved in cold dilute HCl to prepare a 250 $m L$ of solution. Titration of 25.0 $m L$ of this solution requires $12.5 m L of 0.03 M K M n O_{4}$ solution to reach the end point. Number of moles of $F e^{2 +}$ present in 250 $m L$ solution is $x \times 10^{- 2}$ (consider complete dissolution of $F e C l_{2}$ ). The amount of iron present in the sample is $y %$ by weight.
(Assume : $K M n O_{4}$ reacts only with $F e^{2 +}$ in the solution
Use : Molar mass of iron as $56 g m o l^{- 1}$ )

The value of $y$ is .

Open in App

Solution

$Mole of F e^{+ 2} = x \times 10^{- 2} = 1.875 \times 10^{- 2}$
$wt. of F e^{+ 2} = 1.875 \times 10^{- 2} \times 56$
Hence percentage of $F e^{+ 2}$

$= \frac{1.875 \times 10^{- 2} \times 56}{5.6} \times 100 % = 18.75 %$

Suggest Corrections

Similar questions

Q. A sample (5.6 g) containing iron is completely dissolved in cold dilute HCl to prepare a 250

m L

of solution. Titration of 25.0

m L

of this solution requires

12.5 m L of 0.03 M K M n O_{4}

solution to reach the end point. Number of moles of

F e^{2 +}

present in 250

m L

solution is

x \times 10^{- 2}

(consider complete dissolution of

F e C l_{2}

). The amount of iron present in the sample is

y %

by weight.
(Assume :

K M n O_{4}

reacts only with

F e^{2 +}

in the solution
Use : Molar mass of iron as

56 g m o l^{- 1}

)

The value of

y

is .

Q. A

8 g m

sample of iron are containing

V %

(by wt) of iron

F e^{2 +}

was present in

1 L

solution. This solution required

V m L

of a

K M n O_{4}

solution for oxidation of

F e^{2 +}

in acidic medium. If in another titration

20 m L

of same

K M n O_{4}

is required, for oxidation of

20 m L H_{2} O_{2}

in acidic medium. Find volume strength of

H_{2} O_{2}

Q. A

0.46

g sample of

A s_{2} O_{3}

required

25.0

mL of

K M n O_{4}

solution for its titration. The molarity of

K M n O_{4}

solution is :

Q. A 3.4

g

sample of

H_{2} O_{2}

solution containing x% by mass requires

x

ml of a

K M n O_{4}

solution for complete oxidation under acidic medium. The molarity of

K M n O_{4}

solution is:

Q. A 3.4 g sample of

H_{2} O_{2}

solution containing

x % H_{2} O_{2}

by mass requires x mL of a

K M n O_{4}

solution for complete oixidation under acidic condition.The molarity of

K M n O_{4}

solution is:

Join BYJU'S Learning Program

Mole of Fe+2=x×10−2=1.875×10−2 wt. of Fe+2=1.875×10−2×56 Hence percentage of Fe+2 =1.875×10−2×565.6×100%=18.75%

$Mole of F e^{+ 2} = x \times 10^{- 2} = 1.875 \times 10^{- 2}$
$wt. of F e^{+ 2} = 1.875 \times 10^{- 2} \times 56$
Hence percentage of $F e^{+ 2}$

$= \frac{1.875 \times 10^{- 2} \times 56}{5.6} \times 100 % = 18.75 %$