A $1.24 M$ aqueous solution of KI has a density of $1.15 g c m^{- 3}$ .

What is the freezing point of the solution if the KI is completely dissociated in the solution?

- {4.87}^{0} C

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- {3.22}^{0} C

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- {1.22}^{0} C

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{4.87}^{0} C

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Solution

The correct option is A $- {4.87}^{0} C$

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Similar questions

Q. A 1.24 M aqueous solution of KI has density of

1.15 g / c m^{3}

. What is the percentage composition of solute in the solution?

Q. Assertion :When mercuric iodide is added to the aqueous solution of

K I

, the freezing point is raised.
Reason:

H g I_{2}

reacts with

K I

forming complex ion

[H g I_{4}]^{2 -}

Q. Calculate the freezing point of a molar aqueous solution of KCl. (Density of solution =

1.04 g m l^{- 1} K_{f} = 1.86 K k g m o l^{- 1}

)

Q. What is the mass of

K I

in 14.86 mL of a

32.44 g / 100 m L

aqueous

K I

solution?

A 0.1 (M) solution of an acid HA of density 1.01 gm/ml is taken in a beaker. The molecular mass of HA is 300 $g / m o l$ . The freezing point of solution is $0.2087^{o} C$ . For $H_{2} O$ , $K_{f} = 1.86 K / m$

What is the degree of dissociation of HA in its 0.1(M) aqueous solution (in percentage) ?

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A 1.24 M aqueous solution of KI has a density of 1.15 g cm−3.What is the freezing point of the solution if the KI is completely dissociated in the solution?

The correct option is A −4.870C

A $1.24 M$ aqueous solution of KI has a density of $1.15 g c m^{- 3}$ .

What is the freezing point of the solution if the KI is completely dissociated in the solution?

The correct option is A $- {4.87}^{0} C$