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Stoichiometric Calculations

A Sample of m...

Question

A Sample of mixture of $C a C l_{2}$ and $N a C l$ weighing $4.44 g$ was treated to precipitate all the $C a$ as $C a C O_{3}$ , which was then heated and quantitatively converted to $1.12 g$ of $C a O$ . (Atomic weight: Ca= 40, Na= 23, Cl= 35.5)

A

Mixture contains 50%

N a C l

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B

Mixture contains 60%

C a C l_{2}

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C

Mass of

C a C l_{2}

is

2.22 g

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D

Mass of

C a C l_{2}

is

1.11 g

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Solution

The correct option is C Mass of $C a C l_{2}$ is $2.22 g$
Balanced reaction:
$C a C O_{3} 0.02 m o l e △ - \to C O_{2} + C a O 0.02 m o l e$

$C a C l_{2} 0.02 m o l e N a_{2} C O_{3} - ---- \to C a C O_{3} 0.02 m o l e$

mass of $C a C l_{2}$ present in mixture $= 0.02 \times 111 = 2.22 g$ , which is $% 50$ of the total mass, rest being `NaCl`

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Similar questions

Q. A Sample of mixture of

C a C l_{2}

N a C l

4.44 g

was treated to precipitate all the

C a

C a C O_{3}

, which was then heated and quantitatively converted to

1.12 g

C a O

. (Atomic weight: Ca= 40, Na= 23, Cl= 35.5)

Q. A sample of mixture of

C a C l_{2}

N a C l

5.55

g was treated to precipitate all the

C a

C a C O_{3}

which was then heated and quantitatively converted to

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C a C l_{2}

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Q. A sample of a mixture of

C a C l_{2}

N a_{2} C O_{3}

4.22

g was treated to precipitate all the

C a

C a C O_{3}

C a C O_{3}

is heated and quantitatively converted into

0.959

C a O

. Calculate the percentage of

C a C l_{2}

in the mixture.

(Atomic mass of

C a = 40, O = 16, C = 12

C l = 35.5 g / m o l e)

10

g of a sample of a mixture of

C a C l_{2}

N a C l

is treated to precipitate all the calcium as

C a C O_{3}

C a C O_{3}

is heated to convert all the

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and the final mass of

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g. The percent by mass of

C a C l_{2}

in the original mixture is :

10.0

g sample of a mixture of

C a C l_{2}

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is treated to precipitate all the calcium as calcium carbonate. This

C a C O_{3}

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and the final mass of

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X

percentage by mass of

C a C l_{2}

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10 X

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