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:

Hardness of water is $200 \mathrm{ppm}.$ The normality of ${\mathrm{CaCO}}_3$ in the water is in the form of $\mathrm{y}\times {10}^{-3}.$ Identify $\mathrm{y}.$

What is the Relation between ppb and ppm Concentrations?

How to convert 5 % weight/volume to ppb?

How to convert 10 % weight/weight to ppb?

How to convert 10 % Volume/Volume to ppb?

How to convert weight/weight percent to ppm?

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

An aqueous solution of ethanol has strength of $50 \mathrm{g}/\mathrm{L}$. Calculate the weight/weight $(\mathrm{w}/\mathrm{w})\%$ concentration. Given density of pure ethanol $= 0.8 \mathrm{g}/\mathrm{ml}$. And density solution $1 \mathrm{g}/\mathrm{ml}$.

An aqueous solution of ethanol has strength of $50 \mathrm{g}/\mathrm{L}$. Calculate the volume/volume $(\mathrm{V}/\mathrm{V})\%$ concentration. Given density of pure ethanol $= 0.8 \mathrm{g}/\mathrm{ml}$. And density solution $1 \mathrm{g}/\mathrm{ml}$.

An aqueous solution of ethanol has strength of $50 \mathrm{g}/\mathrm{L}$. Calculate the weight/volume $(\mathrm{w}/\mathrm{V})\%$ concentration in $\mathrm{g}/\mathrm{ml}$. Given density of pure ethanol $= 0.8 \mathrm{g}/\mathrm{ml}$. And density solution $1 \mathrm{g}/\mathrm{ml}$.

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)