(1) Calculate the molar solubility of the O2

$\overline{){{\mathbf{S}}}_{{\mathbf{gas}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{{\mathbf{K}}}_{{\mathbf{H}}}{\mathbf{\times}}{{\mathbf{P}}}_{{\mathbf{gas}}}}\phantom{\rule{0ex}{0ex}}{\mathbf{S}}_{{\mathbf{gas}}}\mathbf{}\mathbf{=}\mathbf{}(1.3x{10}^{-3}\frac{M}{\overline{)\mathrm{atm}}})(0.21\overline{)\mathrm{atm}})$

S_{gas }= 2.73x10^{-4 }M

The Henry’s law constant for O_{2 }is 1.3 × 10^{−3} M/atm at 25 °C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 °C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O_{2} is 0.21 atm?

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