If 0.125 L of aqueous solution with a density of 0.810 g/mL contains 13.7 µl of ethanol, epress the concentration of ethanol in ppm, ppb, molarity, molality, and vol%. Pure ethanol has a density of 0.789 g/mL
Molarity = number of moles of solute/per L of solution
=> 2.498 *10^(-4)/0.125 = 1.9984 * 10^(-3) M
Molality = number of moles of solute/per Kg of solvent
Mass of solvent = 810 gm/L * 0.125L = 101.25 gms
Mass of ethanol = 789 gm/L * 13.7 * 10^(-6) L = 0.0108093 gms
molar mass of ethanol = 46 gm/mol
number of moles of ethanol = 0.0108093/46 = 2.498 * 10^(-4) moles
molality = 2.498 * 10^(-4)/(101.25/1000) = 0.00232 m
Volume Percentage = 13.7 * 10^(-6)/0.125 * 100 = 1.0960 * 10^(-2)%
ppm = mg/L = 10.8093/0.125 = 86.4744 ppm
ppb = mg/uL = 86474.4 ppb
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