Average of citric acid per 2-L bottle of soda.

Mass of beaker: 59

Mass of beaker and citric acid: 61

Mass of beaker and citric acid (after cooling): 61.06 or 61.1

Volume of NaOH: 15mL

Mass of citric acid: 2g

Moles of citric acid: 0.0104

(MW = 192.0 g/mol)

Molarity of citric acid: 0.104M

(volume of solution = 100 mL)

Trial 1 equivalence point: 10+7=17/2= 8.5

Trial 2 equivalence point:10+7=17/2=8.5

Molarity (Trial 1):

Molarity (Trial 2):

Average Molarity:

I need help calculating the molarity of the citric acid per trial, please help and show work.

A careless fisherman accidentally spilled an entire 20-oz bottle of soda into Lake Michigan. The soda contained 93.2 mg of caffeine (C8H10N4O2) per 20-oz bottle. What is the resulting molar concentration of caffeine in the lake? Assume that the lake receives no additional caffeine other than from this one bottle of soda; you may also assume that the caffeine is evenly distributed throughout the lake. (Aside: Do you think these assumptions are valid?) Some potentially useful facts about Lake Michigan: Surface area = 5.80 x 104 km2 Average depth = 279 ft Average water density = 1.0 g/mL.