The concentration units which depend on temperature would be

Normality of the solution decreases with increase of temperature, since volume of the solution is directly proportional to temperature.

$Normality=\frac{w}{GEW}\times \frac{1000}{Vinml}$

$Normality\propto \frac{1}{V}$ .

Mass – Mass percentage ((W/W):

$\text{Mass percentage=}\left(\frac{\text{mass of solute}}{\text{mass of solution}}\right)\times 100$

$W\%=\left(\frac{W}{W+W}\right)\times 100$

Molality: The number of moles of the solute present in one Kg (or) 1000g of the solvent.

$m=\frac{W}{GMW}\times \frac{1}{W\left(Kg\right)}$    (or) $m=\frac{W}{GMW}\times \frac{1000}{W\left(g\right)}$

Mole fraction: The ratio between the number of moles of a component of the solution to the total number of moles of all components of the solution is called mole fraction of that component.

Then, mle fraction of solute A is given by  $X_A=\frac{n_A}{n_A+n_B}$  similarly, mole fraction of the solvent B in a solution is

$X_B=\frac{n_B}{n_A+n_B}$

The sum of the mole fractions of all the components in the solution is equal to unity.

$\therefore X_A+X_B=1$

Hence molality, mole fraction and mass percentage these are independent of temperature.