Question

Calculating the amount of Crude Caffeine in mg/L: (0.0173g C8H10N4O2) x (1000mg/1g) x (1/ 0.1L) = 173.0mg/L C8H10N4O2 if it was boiled down to 0.05L, make sure to use the original 0.1L.

Answer 1

To calculate the molarity of a caffeine solution in a 350 mL cup of coffee with 0.150 g of caffeine, you convert the mass of caffeine to moles using its molar mass, then divide by the volume of the solution in liters. The molarity is found to be 0.00221 M.

Step-by-step explanation:

The question asks for the calculation of the molarity of a caffeine solution in a 350 mL cup of coffee that contains 0.150 g of caffeine (C8H10N4O2). To find the molarity, we need to divide the amount of substance (in moles) by the volume of the solution (in liters). First, we determine the molar mass of caffeine. The molar mass of caffeine (C8H10N4O2) is approximately 194.19 g/mol. Using this, we can convert the mass of caffeine into moles:

moles of caffeine = (0.150 g) / (194.19 g/mol) = 0.000772 moles

Then, we convert the volume from milliliters to liters:

volume in liters = 350 mL × (1 L / 1000 mL) = 0.35 L

Now, we can calculate the molarity:

molarity = moles of substance / volume of solution

molarity = (0.000772 moles) / (0.35 L) = 0.00221 M

Thus, the molarity of the caffeine solution in the coffee is 0.00221 M.