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Standard VIII

Chemistry

Solubility

A saturated s...

Question

A saturated solution of iodine in water is $1.25 \times 10^{- 3} (M)$ . In any saturated solution of $I_{2}$ , concentration of $I_{2}$ is $1.25 \times 10^{- 3} (M)$ . In $1 L$ of $0.1 (M)$ solution of $I^{-}$ , it is seen maximum $51.25 \times 10^{- 3} mole$ of $I_{2}$ can be dissolved. In the aqueous solution, $I^{-} (a q), I_{2} (a q)$ undergo complex formation,

What is the value of $K_{C}$ ?

750

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800

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\frac{1000}{51.25}

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Solution

The correct option is B $800$

$K_{C} = \frac{50 \times 10^{- 3}}{50 \times 10^{- 3} \times 1.25 \times 10^{- 3}} = \frac{1000}{1.25} = 800$

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Similar questions

Q. A saturated solution of

I_{2}

in water contains

0.33 g l i t r e^{- 1}

I_{2}

more than this can be dissolved in a

K I

solution because of the following equilibrium:

I_{2} + I^{-} ⇌ I_{3}^{-}

. A

0.1 M K I

solution

(0.1 M I^{-})

actually dissolves

12.5 g / l i t r e I_{2}

, most of which is converted to Assuming that the concentration of

I_{2}

in all saturated solution is the same, calculate the equilibrium constant

(K_{c})

for the above reaction. What is the effect of adding water to clear saturated solution of

I_{2}

K I

solution.

Q. A saturated solution of iodine in water contains

0.33

g iodine/L. More than this can dissolve in a

K I

solution because of the following equilibrium:

I_{2} (a q) + I^{-} \to I_{3} - (a q)

. A

0.1 M

K I

solution

(0.1 M

I^{-})

actually dissolves

12.5

g of Iodine/L, most of which is converted to

I_{3}^{-} .

Assuming that the concentration of

I_{2}

in all saturated solutions is the same, calculate the equilibrium constant for the above reaction: (Mol. wt. of

I

258 g m o l^{- 1}

)

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Q. In

1 L

saturated solution of

A g C l [K_{s p} = 1.6 \times 10^{- 10}]

0.01 m o l e o f C u C l [K_{s p} = 1 \times 10^{- 6}]

is added. The resultant concentration of

A g^{+}

in the solution is

1.6 \times 10^{- x} M

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Q. Enough

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is dissolved in water at 298 K to produce a saturated solution. The concentration of

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The correct option is B 800 KC=50×10−350×10−3×1.25×10−3=10001.25=800

The correct option is B $800$

$K_{C} = \frac{50 \times 10^{- 3}}{50 \times 10^{- 3} \times 1.25 \times 10^{- 3}} = \frac{1000}{1.25} = 800$