Suppose you are a food chemist working for a company that makes and manufactures soda. Your job is to create a new soft drink wi
th the ingredients available to you. There is one problem—you need 1 liter of phosphoric acid solution, and the phosphoric acid available to use has a concentration of 0.01 M. This is much too high to add to your soda without distorting the flavor. Typically, there are about 45 milligrams of phosphoric acid per 12 ounce can of soda. Here is your task: Convert the 45 milligrams of phosphoric acid (H3PO4) into grams and then into moles.
0.00046 moles or 4.6×10-4 moles
Given that 12 ounces is equal to about 0.35 liter, find the molarity of the phosphoric acid in a typical can of soda (45 milligrams). 0.0013 M or 1.3×10-3 M
Using the dilution equation, determine how much of the stock solution (0.01 M H3PO4) you will need to make 1 liter of the concentration typically used in soda.
0.13 liter or 130 milliliters
The stoichiometry of the reaction gives the molar ratio in which the reactants react with each other and the ratio in which products are formed. The coefficients of the reactants in the reaction follow the stoichiometry the balanced chemical equation for the reaction is as follows; 2C₃H₆(g) + 9O₂(g) ---> 6CO₂(g) + 6H₂O(l)
