(B) $1 \ ppm$ (part per million) by mass means $1 \ part$ of solute in $10^6 \ parts$ of solution by mass. Given,concentration of $CHCl_3 = 15 \ ppm$.

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(B) $1 \ ppm$ (part per million) by mass means $1 \ part$ of solute in $10^6 \ parts$ of solution by mass. Given,concentration of $CHCl_3 = 15 \ ppm$. This means $15 \ g$ of $CHCl_3$ is present in $10^6 \ g$ of the water sample. Percentage by mass $= \frac{\text{Mass of solute}}{\text{Mass of solution}} \times 100$. Percentage by mass $= \frac{15}{10^6} \times 100 = 15 \times 10^{-4} = 1.5 \times 10^{-3} \%$.

Class 12 Chemistry Solutions Method of expressing concentration of solution

Medium

$A$ sample of drinking water is found to be severely contaminated with chloroform $(CHCl_3)$,which is a suspected carcinogen. If the level of contamination is $15 \ ppm$ (by mass),express this in percentage by mass.

A
$1.6 \times 10^{-2}$
B
$1.5 \times 10^{-3}$
C
$1.8 \times 10^{-2}$
D
$1.9 \times 10^{-2}$

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Method of expressing concentration of solution

The density of a $3 \, M \, NaCl$ solution is $1.25 \, g \, mL^{-1}$. Calculate the molality of the solution. (in $, m$)

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$A$ commercially sold concentrated $HCl$ is $35 \%$ $HCl$ by mass. If the density of this commercial acid is $1.46 \ g/mL$,the molarity of this solution is $....M$.
(Atomic mass : $Cl = 35.5 \ amu, H = 1 \ amu$)

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The molarity of $20\% \,(W/W)$ solution of sulphuric acid is $2.55 \, M$. The density of the solution is $........... \, g \, cm^{-3}$.

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$200 \, mL$ of $0.6 \, N$ $H_2SO_4$ and $100 \, mL$ of $0.3 \, N$ $HCl$ are mixed together. The acidic normality of the resultant solution is $........ N$.

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What is meant by a binary solution?

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$A$ sample of drinking water is found to be severely contaminated with chloroform $(CHCl_3)$,which is a suspected carcinogen. If the level of contamination is $15 \ ppm$ (by mass),express this in percentage by mass.

Similar Questions

The density of a $3 \, M \, NaCl$ solution is $1.25 \, g \, mL^{-1}$. Calculate the molality of the solution. (in $, m$)

$A$ commercially sold concentrated $HCl$ is $35 \%$ $HCl$ by mass. If the density of this commercial acid is $1.46 \ g/mL$,the molarity of this solution is $....M$.(Atomic mass : $Cl = 35.5 \ amu, H = 1 \ amu$)

The molarity of $20\% \,(W/W)$ solution of sulphuric acid is $2.55 \, M$. The density of the solution is $........... \, g \, cm^{-3}$.

$200 \, mL$ of $0.6 \, N$ $H_2SO_4$ and $100 \, mL$ of $0.3 \, N$ $HCl$ are mixed together. The acidic normality of the resultant solution is $........ N$.

What is meant by a binary solution?

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$A$ commercially sold concentrated $HCl$ is $35 \%$ $HCl$ by mass. If the density of this commercial acid is $1.46 \ g/mL$,the molarity of this solution is $....M$.
(Atomic mass : $Cl = 35.5 \ amu, H = 1 \ amu$)