The density of a $1.0 \, m$ aqueous solution of glucose is $1.1 \, g/mL$. What is the molarity of the solution in $M$?

What is the mole fraction of the solute in $2.5 \ m$ aqueous solution?

The strength of a solution $(S)$ in $g/L$ is related to its normality $(N)$ and equivalent weight $(E)$ of the solute by the formula:

How many $cc$ of water should be added to $200 \ cc$ of $seminormal$ $NaOH$ solution to make it $decinormal$?

What is the mole fraction of the solute in a $2.5 \, m$ aqueous solution?

Commercially available $H_2SO_4$ is $98 \ g$ by weight of $H_2SO_4$ and $2 \ g$ by weight of water. Its density is $1.38 \ g \ cm^{-3}$. Calculate the molality $(m)$ of $H_2SO_4$ (molar mass of $H_2SO_4$ is $98 \ g \ mol^{-1}$). (in $m$)