The density of a $10.0\% \, w/w$ aqueous solution of $KCl$ is $1.06 \, g \, cm^{-3}$. The molarity of this solution is ........

$A$ $2.0 \, M$ solution is obtained when $0.5 \, mole$ of solute is dissolved in:

$3.1 \ g$ of a compound,'$X$' (molar mass $= 62 \ g \ mol^{-1}$) is dissolved in $19.5 \ g$ of other compound,$Y$ (molar mass $= 78 \ g \ mol^{-1}$). The ratio of mole fractions of $X$ and $Y$ in the solution is

The molality of a solution is defined as:

How are $0.50 \, mol$ $Na_{2}CO_{3}$ and $0.50 \, M$ $Na_{2}CO_{3}$ different?

You are supplied with $500 \ mL$ each of $2 \ N \ HCl$ and $5 \ N \ HCl$. What is the maximum volume of $3 \ M \ HCl$ that you can prepare using only these two solutions (in $mL$)?