Concentration Terms

Commercially available concentrated hydrofluoric acid contains $38\% \mathrm{HF}$ by volume$\left(\raisebox{1ex}{$\mathrm{v}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{V}$}\right.\%\right)$. The density of $\mathrm{HF}$ is $1.19 \mathrm{g} {\mathrm{ml}}^{-1}$ and density of solution is $1.39 \mathrm{g} {\mathrm{ml}}^{-1}$. What is the molality of this solution?
 

Commercially available concentrated hydrofluoric acid contains $48\% \mathrm{HF}$ by volume$\left(\raisebox{1ex}{$\mathrm{v}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{V}$}\right.\%\right)$. What is the molality of this solution? The density of $\mathrm{HF}$ is $1.19 \mathrm{g} {\mathrm{ml}}^{-1}$ and density of solution is $1.39 \mathrm{g} {\mathrm{ml}}^{-1}$.
 

Commercially available concentrated hydrofluoric acid contains $48\% \mathrm{HF}$ by volume$\left(\raisebox{1ex}{$\mathrm{v}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{V}$}\right.\%\right)$. What is the molality of this solution? The density of $\mathrm{HF}$ is $1.19 \mathrm{g} {\mathrm{ml}}^{-1}$ and density of solution is $1.39 \mathrm{g} {\mathrm{ml}}^{-1}$.
 

Commercially available concentrated hydrochloric acid contains $28\% \mathrm{HCl}$ by volume$\left(\mathrm{v}/\mathrm{V}\%\right)$. The density of $\mathrm{HCl}$ is $3.131 \mathrm{g} {\mathrm{ml}}^{-1}$. The molarity of the solution is $\approx 24 \mathrm{M}$
 

Commercially available concentrated hydrochloric acid contains $28\% \mathrm{HCl}$ by volume$\left(\mathrm{v}/\mathrm{V}\%\right)$. The density of $\mathrm{HCl}$ is $3.131 \mathrm{g} {\mathrm{ml}}^{-1}$. The molarity of the solution is
 

Commercially available concentrated hydrochloric acid contains $28\% \mathrm{HCl}$ by volume. What is the molarity of this solution? The density of $\mathrm{HCl}$ is $3.131 \mathrm{g} {\mathrm{ml}}^{-1}$.
 

(Weight/weight)% $= \mathrm{d} \times$ (volume/weight)%

A $20\% (\mathrm{v}/\mathrm{W})$ solution has a density of $1.5 \mathrm{g}/\mathrm{ml}$. The weight percentage$(\mathrm{w}/\mathrm{W}\%)$ of the solution is $30\%$.

A $15\% (\mathrm{v}/\mathrm{W})$ solution has a density of $1.5 \mathrm{g}/\mathrm{ml}$. Calculates the weight percentage$(\mathrm{w}/\mathrm{W}\%)$ of the solution.

 The molarity of urea solution containing $6.02\times {10}^{20}$ molecules of urea are present in $100\mathrm{ml}$ of its solution is

Commercially available concentrated hydrofluoric acid contains $38\% \mathrm{HF}$ by volume$\left(\raisebox{1ex}{$\mathrm{v}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{V}$}\right.\%\right)$. What is the molality of this solution? The density of $\mathrm{HF}$ is $1.19 \mathrm{g} {\mathrm{ml}}^{-1}$ and density of solution is $1.39 \mathrm{g} {\mathrm{ml}}^{-1}$.
 

Commercially available concentrated hydrochloric acid contains $38\% \mathrm{HCl}$ by volume. What is the molarity of this solution? The density of $\mathrm{HCl}$ is $3.131 \mathrm{g} {\mathrm{ml}}^{-1}$.
 

What is relation between weight/weight and volume/weight concentrations?

The amount of ${\mathrm{H}}_2{\mathrm{O}}_2$ present in $1 \mathrm{L}$ of $1.5 \mathrm{N} {\mathrm{H}}_2{\mathrm{O}}_2$ solution is

The concentration of a solution is $4\%(\mathrm{w}/\mathrm{w})$ and $10\%(\mathrm{w}/\mathrm{v})$. Calculate density $(\mathrm{in} \mathrm{g}/\mathrm{ml})$ of solution.

The concentration of a solution is $6\%(\mathrm{w}/\mathrm{w})$ and $10\%(\mathrm{w}/\mathrm{v})$. Calculate density $(\mathrm{in} \mathrm{g}/\mathrm{ml})$ of solution.

The concentration of a solution is $8\%(\mathrm{w}/\mathrm{w})$ and $10\%(\mathrm{w}/\mathrm{v})$. Calculate density $(\mathrm{in} \mathrm{g}/\mathrm{ml})$ of solution.

A substance that dissolves a solute to form a solution is called as: