Final answer:
The molar concentration of anthracene in the well water sample, having a concentration of 15.52ppb and a water density of 1.00g/mL, is 8.71 × 10^-11 mol/L.
Step-by-step explanation:
To calculate the molar concentration of anthracene in a well water sample with a concentration of 15.52ppb, first, understand that 'ppb' stands for 'parts per billion'. Since the density of the water sample is given as 1.00g/mL, we can assume that 1 liter of water weighs 1000g, and thus 15.52ppb is equivalent to 15.52ug (micrograms) of anthracene per liter of water.
Next, we will convert the mass of anthracene to moles by using its molar mass (178.23 g/mol).
Moles of anthracene = Mass of anthracene / Molar mass of anthracene
Moles of anthracene = (15.52 × 10^-6 g) / (178.23 g/mol)
Finally, the molarity (M) is the number of moles per liter:
Molarity of anthracene = Moles of anthracene / Volume (in liters)
Molarity of anthracene = (15.52 × 10^-6 g) / (178.23 g/mol) / 1 L
By doing the calculation:
Molarity of anthracene = 8.71 × 10^-11 mol/L