What is the mole fraction of the solute in a $1 \, m$ (molal) aqueous solution?

$A$ solution of sodium sulphate contains $92 \ g$ of $Na^{+}$ ions per kilogram of water. The molality of $Na^{+}$ ions in that solution in $mol \ kg^{-1}$ is:

An aqueous solution of glucose is $10\%$ in strength. The volume in which $1 \, \text{g-mole}$ of it is dissolved will be ........... $L$.

In $500 \ mL$ of $0.2 \ M \ NaCl$ solution,$1500 \ mL$ of $0.4 \ M \ MgCl_2$ solution is mixed. The only incorrect final concentration of ion is (assume volume to be additive)

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

$25.3 \ g$ of sodium carbonate,$Na_2CO_3$ is dissolved in enough water to make $250 \ mL$ of solution. If sodium carbonate dissociates completely,the molar concentration of sodium ions,$Na^{+}$,and carbonate ions,$CO_3^{2-}$,are respectively:
(Molar mass of $Na_2CO_3 = 106 \ g \ mol^{-1}$)