The density of $NH_4OH$ solution is found to be $0.6 \, g/mL$. It contains $35 \%$ by mass of $NH_4OH$. The normality of the solution is ......... $N$.

Sea water,which can be considered as a $6 \ M$ solution of $NaCl$,has a density of $2 \ g \ mL^{-1}$. The concentration of dissolved oxygen $(O_2)$ in sea water is $5.8 \ ppm$. Then the concentration of dissolved oxygen $(O_2)$ in sea water is $x \times 10^{-4} \ m$. $x = ............$ $(Nearest \ integer)$
Given: Molar mass of $NaCl$ is $58.5 \ g \ mol^{-1}$. Molar mass of $O_2$ is $32 \ g \ mol^{-1}$.

The approximate molarity of a solution in $mol \ L^{-1}$ that contains $13.50 \ g$ of $NaCl$ dissolved in $452 \ mL$ of water is

The molality of a $10\%\ (v/v)$ solution of di-bromine in $CCl_4$ (carbon tetrachloride) is $x$. $x = ...... \times 10^{-2}\ m$. (Nearest integer)
[Given : molar mass of $Br_2 = 160\ g\ mol^{-1}$
atomic mass of $C = 12\ g\ mol^{-1}$
atomic mass of $Cl = 35.5\ g\ mol^{-1}$
density of dibromine $= 3.2\ g\ cm^{-3}$
density of $CCl_4 = 1.6\ g\ cm^{-3}$]

$A$ solution of glucose in water is labelled as $10 \% \ w/w$. What would be the molality and mole fraction of each component in the solution? If the density of the solution is $1.2 \ g \ mL^{-1}$,then what shall be the molarity of the solution?

Which of the following modes of expressing concentration is independent of temperature?