Concentration Terms

Specific volume of a cylindrical virus particle whose radius and length are $7 \mathrm{\AA }$ and $10 \mathrm{\AA }$ respectively, is  $6.02\times {10}^{-2}\mathrm{cc}/\mathrm{g}$. If  ${\mathrm{N}}_{\mathrm{A}}=6.02\times {10}^{23}$, find the molecular weight of the virus:

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 $3.131 \mathrm{g} {\mathrm{ml}}^{-1}$.
 

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 $3.131 \mathrm{g} {\mathrm{ml}}^{-1}$.
 

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

The mole-fraction of a solute in one molal ethanolic solution would be (Given, molecular mass of ethanol $=46.07 \mathrm{g}.{\mathrm{mol}}^{-1}$ )

In ${\mathrm{Fe}}_{0.96}\mathrm{O},\mathrm{Fe}$ is present in $+2$ and $+3$ oxidation state, what is the mole-fraction of ${\mathrm{Fe}}^{2+}$ in the compound?

Calculate the amount of oxalic acid $\left({\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4.2{\mathrm{H}}_2\mathrm{O}\right)$ required to obtain $250\mathrm{ }\mathrm{m}\mathrm{L}$ of deci-molar solution.

An antifreeze solution is prepared from $222.6\mathrm{ }\mathrm{g}$ of ethylene glycol $\left[{\mathrm{C}}_2{\mathrm{H}}_4{\left(\mathrm{O}\mathrm{H}\right)}_2\right]$ and $200\mathrm{ }\mathrm{g}$ of water. If the density of the solution is $1.072\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{m}{\mathrm{L}}^{-1}$ then what shall be the molarity of the solution?

Find the molality of ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$ solution whose specific gravity is $1.98\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{m}{\mathrm{L}}^{-1}$ and $90\mathrm{\%}$ weight by volume ${\mathrm{ }\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$.