What is the "molality" of a 4.00*g mass of sodium chloride dissolved in 100*mL of water?

$\text{Molality"-="Moles of solute"/"Kilograms of solvent} \cong 0.7 \cdot m o l \cdot k {g}^{-} 1$
And so here "molality"=((4.00*g)/(58.44*g*mol^-1))/(100*gxx10^-3*kg*g^-1)=??*mol*kg^-1.
At these concentrations, $\text{molality}$ would be little different to $\text{molarity"="Moles of solute"/"Litres of solution}$