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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 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.

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 E $0.40 M$
$A g N O_{3} + N a C l \to A g C l + N a N O_{3}$
The molar mass of AgCl is $108 + 35.5 = 143.5$ g/mol.
5.7 g AgCl corresponds to $\frac{5.7 g}{143.5 g / m o l} = 0.040 m o l$ .
The number of moles of $A g^{+}$ ions is equal to the number of moles of AgCl. It is 0.040 moles
The molar concentration is the ratio of the number of moles of $A g^{+}$ ions to total volume of solution in L.
It is $\frac{0.040 m o l}{100 m L \times \frac{100 m L}{1000 m L}} = 0.40$ M.

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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 -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?

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

A g C l

was precipitated. The value of

x

is:

Q. A

1.5

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

250

mL. A

20

mL portion of this solution was then mixed with

30

mL of an alkali solution. The resulting solution was then treated with stoichiometric amount of

C a C l_{2}

just needed for precipitation of oxalate as

C a C_{2} O_{4}

solution was filtered off and filtrate was finally titrated against

0.1 M H C l

solution.

8.0

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

A g N O_{3}

solution and

A g C l

obtained was washed, dried and weighed to be

0.4305

g. Determine the mass percentage of oxalic acid in the original sample.

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

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.