When the concentration is expressed as the number of moles of a solute per litre of solution,it is known as:

The molarity of $20\% \,(W/W)$ solution of sulphuric acid is $2.55 \, M$. The density of the solution is $........... \, g \, cm^{-3}$.

What is the mole fraction of the solute in a $1.00 \, m$ aqueous solution?

What is meant by mass percentage $( \% w/w )$?

If the density of a $2.05 \ M$ $CH_3COOH$ solution is $1.02 \ g/mL$,what is the molality of the solution?

$A$ commercially sold concentrated $HCl$ is $35 \%$ $HCl$ by mass. If the density of this commercial acid is $1.46 \ g/mL$,the molarity of this solution is $....M$.
(Atomic mass : $Cl = 35.5 \ amu, H = 1 \ amu$)