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Stoichiometric Calculations

A 100 -millil...

Question

A 100 -milliliter solution of $A g N O_{3}$ and excess $N a C l$ were treated and the silver was precipitate as $A g C l$ . If 5.7 g $A g C l$ was obtained, what was the concentration of Ag $^{+}$ in the original solution?

0.03

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0.05

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0.12

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0.30

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0.40

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Solution

The correct option is E $0.40$ M
The molar mass of $A g C l$ is $108 + 35.5 = 143.5$ g/mol.
Number of moles is the ratio of mass to molar mass.
Number of moles of $A g C l$ $= \frac{5.7 g}{143.5 g / m o l} = 0.0397$ moles.
0.0397 moles of $A g C l$ are obtained from 0.0397 moles of $A g^{+}$ .
Molarity of $A g^{+} = \frac{0.0397 m o l}{0.100 L} = 0.4 M$
Hence, the option (E) is the correct answer.

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Similar questions

Q. A 100-milliliter 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?

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

mL solution containing

A g N O_{3}

was treated with excess of

N a C l

to precipitate the silver as

A g C l

completely. Determine the

{A g}^{+}

concentration in original solution, if

5.7 g

A g C l

was obtained.

x

g of

A g

was dissolved in

H N O_{3}

and the solution was treated with excess of

N a C l

. When

2.87

g of

A g C l

was precipitated, the value of

x

is :

Q. What is the concentration of

A g^{+}

ion in

0.01 M A g N O_{3}

that is also

1.0 M N H_{3}

?
Will

A g C l

precipitate from a solution that is

0.01 M A g N O_{3}

0.01 M N a C l

and

1 M N H_{3}

?
Given : Formation constant,

K_{f} o f [A g (N H_{3})_{2}]^{+} = 1.70 \times 10^{7} a n d K_{s p} A g C l = 1.8 \times 10^{- 10}

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A 100 -milliliter solution of AgNO3 and excess NaCl were treated and the silver was precipitate as AgCl . If 5.7 g AgCl was obtained, what was the concentration of Ag+ in the original solution?

A 100 -milliliter solution of $A g N O_{3}$ and excess $N a C l$ were treated and the silver was precipitate as $A g C l$ . If 5.7 g $A g C l$ was obtained, what was the concentration of Ag $^{+}$ in the original solution?