Single Choice

In which mode of expression, the concentration of a solution remains independent of temperature?

AMolarity
BNormality
CFormality
DMolality
Correct Answer

Solution

Molality of a solution is defined as number of moles of solute present in 1.0 kg (1000 g) of solvent.
$$Molality (m) = \dfrac {moles \ of\ solute} {Mass\ of \ solvent (in\ kg)}$$
Thus, the expression for molality contains weights. It does not contain volume terms. Hence, it is independent of the temperature of the solution.
Molarity, normality and formality contains volume terms. Hence, they depend on temperature.

SIMILAR QUESTIONS

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Mole Concept

The density of $$1$$ M solution of $$NaCl$$ is $$1.0585\:g\:ml^{-1}$$. The molality of the solution is :

Mole Concept

If $$20\:mL$$ of ethanol (density$$=\,0.7893\:g/mL$$) is mixed with $$40\:mL$$ water (density$$=\,0.9971\:g/mL$$) at $$25^{\circ}C$$, the final solution has density of $$0.9571\:g/mL$$. Calculate the molality of alcohol in the final solution. (as nearest integer)

Mole Concept

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Mole Concept

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Mole Concept

3 g of salt having molecular weight 30 is dissolved in 250 g of water. The molality of the solution is:

Mole Concept

A compound H$$_2$$X with molar weight of 80g is dissolved in a solvent having density of 0.4 gml$$^{-1}$$. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution is:

Mole Concept

The mole fraction of urea in aqueous urea containing $$900\ g$$ of water is $$0.05$$. If the density of the solution is $$1.2\ g/cm^3$$, the molarity of urea solution is ______.

Mole Concept

The molality of the solution containing 15.20 g of urea (molar mass = 60) dissolved in 150 g of water is:

Mole Concept

An aqueous solution of urea containing 18g urea in 1500 cm$$^3$$ of the solution has a density equal to 1.052. If the molecular weight of urea is 60, the molality of the solution is:

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