Molality of $0.8 \ M \ H_2SO_4$ solution (density $1.06 \ g \ cm^{-3}$) is . . . . . . $\times 10^{-3} \ m$.

The molality of $648 \ g$ of pure water is .................. $m$.

$A$ certain aqueous solution of $FeCl_3$ (formula mass $= 162 \ g/mol$) has a density of $1.1 \ g/mL$ and contains $20.0 \ \% \ FeCl_3$ by mass. The molar concentration (molarity) of this solution is: (in $M$)

Calculate the mole fraction of solute in the solution if the solution is prepared by dissolving $394 \ g$ of a nonvolatile solute in $622 \ g$ of water at $30^{\circ}C$ (Molar mass of solute $= 342 \ g \ mol^{-1}$).

If $5 \ g$ $NaOH$ is dissolved in $450 \ mL$ of solution,the molarity of the solution is: $(Na=23, O=16, H=1 \ g \ mol^{-1})$ (in $M$)

The density of $NaOH$ solution is $1.2 \, g \, cm^{-3}$. The molality of this solution is $.... \, m$ (Round off to the nearest integer). [Use: Atomic masses: $Na: 23.0 \, u, O: 16.0 \, u, H: 1.0 \, u$]