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 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 $1.39 \mathrm{g} {\mathrm{ml}}^{-1}$.
 

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 ${\mathrm{ }\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$.

In the case of 2 molal aqueous solution of sulphuric acid, calculate the mole fraction of the solvent:

The molarity of $0.56 \mathrm{L}$ of water vapour at $\mathrm{STP}$ is:

Zinc can be determined volumetrically by the precipitation reaction as given below

$3{\mathrm{Zn}}^{2+}+2\left[{\mathrm{K}}_4\mathrm{Fe}(\mathrm{CN}{)}_6^{}\right]⟶{\mathrm{K}}_2{\mathrm{Zn}}_3{\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]}_2+6{\mathrm{K}}^{+}$

A sample of zinc ore weighing $1.5432 \mathrm{g}$ was prepared for the reaction and required $34.68 \mathrm{mL}$ of $0.1043 \mathrm{M} {\mathrm{K}}_4\mathrm{Fe}{\left(\mathrm{CN}\right)}_6$ for titration. The mass percentage of zinc in the ore is (report the value in the nearest integer)

A commercial sample $(2.013 \mathrm{g})$ of $\mathrm{NaOH}$ containing ${\mathrm{Na}}_2{\mathrm{CO}}_3$ as an impurity was dissolved to give $250 \mathrm{mL}$ of solution. A $10 \mathrm{mL}$ portion of the solution required $20 \mathrm{mL}$ of $0.1 \mathrm{N} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution for complete neutralisation. Calculate the percentage by weight of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ in the sample. (Express your answer by multiplying with 1000 and rounding off to three significant figures)