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Standard XII

Chemistry

Molarity

4.0 g of a mi...

Question

4.0 g of a mixture of NaCl and an unknown metal iodide $M I_{2}$ was dissolved in a water to form its aqueous solution. To this aqueous solution, The aqueous solution $A g N O_{3}$ was added gradually so that silver halides are precipitated. The precipitates were weighed at regular interval and the given curve for the mass of precipitate versus volume of $A g N O_{3}$ added was obtained. With the knowledge of the fact that halides are precipitated successively i.e., when one halide is precipitating , the other halide remains in the solution, answer the following questions:
(Molar mass of Ag = 108, I = 127, Na = 23).
Points p and Q are: P(20, 4.8), Q(37, 7.25),
What is the approximate molarity of $A g N O_{3}$ solution?

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Solution

The correct option is C 1
Volume of ${A g N O}_{3}$ for $N a C l = 37 - 20 = 17 m L$
(from fig. graph) momol of $Agc 1$ formed $= \frac{2.45}{143.5} \times 1000 = 17 m m o l$
$\Rightarrow 17 m m o l {A g N O}_{3}$ is present in $17 m L$ solution
$\begin{matrix} Hence, molarity = mole/ volume = \frac{17}{17} = 1.0 M \end{matrix}$
Hence (C) is correct option.

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Similar questions

Q. 4.0 g of a mixture of

N a C l

and an unknown metal iodide

M I_{2}

was dissolved in a water to form its aqueous solution. To this aqueous solution, The aqueous solution

A g N O_{3}

was added gradually so that silver halides are precipitated. The precipitates were weighed at regular interval and the given curve for the mass of precipitate versus volume of

A g N O_{3}

added was obtained. With the knowledge of the fact that halides are precipitated successively i.e. when one halide is precipitating , the other halide remains in the solution, answer the following questions:
(Molar mass of

A g = 108, I = 127, N a = 23

).
Points

P

and

Q

are:

P (20, 4.8), Q (37, 7.25)

What is the approximate mass percentage of

M I_{2}

Q. In order to determine the composition of a mixture of halides containing

M B r_{2}

and

N a l, 14

g mixture was dissolved in water. To this solution,

A g N O_{3}

solution of certain molarity was added gradually. The mass of precipitate produced (in g) were measured and it was plotted against volume of

A g N O_{3}

solution added (in ml). Its known that

A g I

is precipitated first. Precipitation of

B r

does not start until the already precipitating

I^{-}

precipitates completely. Find out the value of

A B \times C D

where:

A B

=

Atomic weight of metal

M

C D

=

Mole percent of

N a l

in original mixture.

Q. A colourless aqueous solution contain nitrates of two metal, when it is added to an aqueous solution of

N a C l

, a white precipitate ws formed. This precipitate was found to be partially soluble in hot water to give a residue

P

and a solution

Q

. The residue

P

was solublein aq. in

N H_{3}

and also in excess sodium thiosulfate. The hot solution

Q

gave a yellow precipitate with

K I

. The metals

X

and

Y

, respectively, are:

A g N O_{3}

(aq) was added to an aqueous

K C l

solution gradually and the conductivity of the solution was measured. The plot of conductance

(Λ)

versus the volume of

A g N O_{3}

is :

Q. Explain the following :
(i) When

N a C l

is added to

A g N O_{3}

solution, a white precipitate is formed.
(ii) An aqueous solution of ammonium chloride is acidic in nature.

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The correct option is C 1Volume of AgNO3 for NaCl=37−20=17 mL(from fig. graph) momol of Agc1formed =2.45143.5×1000=17mmol⇒17mmolAgNO3 is present in 17 mL solution Hence, molarity = mole/ volume =1717=1.0MHence (C) is correct option.