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Standard XII

Chemistry

Stoichiometric Calculations

A 100 ml so...

Question

A $100$ ml solution containing $A g N O_{3}$ was treated with excess $N a C l$ to completely precipitate the silver as $A g C l$ . If $5.7$ g $A g C l$ was obtained, what was the concentration of $A g^{+}$ in the original solution?

0.03 M

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0.05 M

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0.12 M

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0.30 M

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0.40 M

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Solution

The correct option is D $0.40 M$
The molecular weight of $A g C l$ is $108 + 35.5 = 143.5$ g/mol.

5.7 g $A g C l$ corresponds to $\frac{5.7 g}{143.5 g / m o l} = 0.03972$ moles.

0.03972 moles of $A g C l$ are obtained from 0.03972 moles of $A g N O_{3}$ .
The volume of $A g N O_{3}$ is 100 ml or 0.100 L.

$[A g N O_{3}] = \frac{0.03972 m o l}{0.100 L} = 0.3972 M ≃ 0.40 M$

Hence, the concentration of $A g^{+}$ in the original solution was 0.40 M.

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Similar questions

Q. A

100 m L

solution containing

A g N O_{3}

was treated with excess

N a C l

to completely precipitate the silver as

A g C l

. If

5.7 g A g C l

was obtained, what was the concentration of

A g^{+}

in the original solution? (At. mass of

A g = 108 g / m o l

)

Q. A 100 -milliliter solution of

A g N O_{3}

and excess

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were treated and the silver was precipitate as

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. If 5.7 g

A g C l

was obtained, what was the concentration of Ag

^{+}

in the original solution?

x

g of

A g

was dissolved in

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and the solution was treated with excess of

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. When

2.87

g of

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was precipitated, the value of

x

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Q. A

1.5

g sample containing oxalic acid and some inert impurity was dissolved in enough water and volume was made up to

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mL portion of this solution was then mixed with

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just needed for precipitation of oxalate as

C a C_{2} O_{4}

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mL of acid was required to reach the equivalence point. At last the above neutral solution was treated with excess of

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Q. 5.85 g of

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[Atomic mass of

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N a = 23

u and

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A 100 ml solution containing AgNO3 was treated with excess NaCl to completely precipitate the silver as AgCl. If 5.7 g AgCl was obtained, what was the concentration of Ag+ in the original solution?

A $100$ ml solution containing $A g N O_{3}$ was treated with excess $N a C l$ to completely precipitate the silver as $A g C l$ . If $5.7$ g $A g C l$ was obtained, what was the concentration of $A g^{+}$ in the original solution?