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Standard IX

Chemistry

Ways of Representing the Concentration of a Solution

What concentr...

Question

What concentration of nitrogen should be present in a glass of water at room temperature? Assume a temperature of $25^{o}$ C, a total pressure of $1$ atmosphere and mole fraction of nitrogen in air of $0.78$ . ( $K_{H}$ for nitrogen $= 8.42 \times 10^{- 7}$ M/mm Hg).

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Solution

$p_{N_{2}} = 1 a t m$
$p_{N_{2}} = K_{H} \times N_{2}$
By using Henry's Law
$x N_{2} = \frac{p_{N_{2}}}{K_{H}} = \frac{1}{8.42 \times 10^{- 7}}$
$= \frac{n (N_{2})}{n (H_{2} O)}$
$= x N_{2} . n (H_{2} O)$
$= x N_{2} . \frac{1000}{18}$
$= \frac{1}{8.42 \times 10^{- 7}} \times 55.5$
$= 6.59 \times 10^{7} m o l e s$
Hence Nitrogen concentration
$= 6.59 \times 10^{7} m o l L^{- 1}$

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What concentration of nitrogen should be present in a glass of water at room temperature? Assume a temperature of 25oC, a total pressure of 1 atmosphere and mole fraction of nitrogen in air of 0.78. (KH for nitrogen =8.42×10−7M/mm Hg).

pN2=1atmpN2=KH×N2By using Henry's Law xN2=pN2KH=18.42×10−7=n(N2)n(H2O)=xN2.n(H2O)=xN2.100018=18.42×10−7×55.5=6.59×107molesHence Nitrogen concentration =6.59×107molL−1

What concentration of nitrogen should be present in a glass of water at room temperature? Assume a temperature of $25^{o}$ C, a total pressure of $1$ atmosphere and mole fraction of nitrogen in air of $0.78$ . ( $K_{H}$ for nitrogen $= 8.42 \times 10^{- 7}$ M/mm Hg).