Question

Question:1 If an Alka-Seltzer tablet contained 300. mg of aspirin, 1.905 x 1003 mg of sodium hydrogen carbonate (also known as sodium bicarbonate), and 1.025 x 1003 mg of citric acid and nothing else, what is the percent, by mass, of sodium hydrogen carbonate in the tablet?

Question:2 Using the tablet information from Question 1, calculate the moles of CO2 you would theoretically expect from 0.202 grams of an Alka-Seltzer tablet at 715 torr and 292 K.

Question:3 You conduct an experiment where N2 is collected over water in a 1.03 L flask at 17oC. At the conclusion of the experiment, the total pressure in the flask is 568 torr. What is the pressure of N2 in the flask?

Question:4 A student reacted a sample of NaHCO3 with acid under the same conditions that will be used in lab. The total volume of gas collected plus the correction factor was 50.1 mL at a total pressure of 672 torr and 25oC. How many moles of CO2(g) were produced?

Answer 1

There are too many questions ....four questions and each involves calculations so please post separately....

i am solving 1 and   2 only.....

1)          Aspirin Formula‎: ‎C₉H₈O₄                    Mass of aspirin = 300 mg

citric acid Formula: C₆H₈O₇          mass of citric acid = 1025 mg

             NaHCO₃                                        Mass of NaHCO₃ = 1905 mg

      % of NaHCO₃    = {(Mass of NaHCO₃ ) / total mass of all sample} x100

                                =   {(1905)/ (1025+1905+300) }x100 = 58.9 %

2) Assuming all the carbon is extracted from the tablet and converted to CO₂

citric acid Molar mass: 192. 0 g/mol , aspirin Molecular mass‎: ‎180.0 g/mol

   NaHCO3 Molar mass = 84g/mol

   Millimoles of Carbon per tablet   = 9 x 300/180    + 6 x 1025/192    + 1 x 1905/84

                                                     = 15 +   32 + 22.67 millimoles = 69.67 millimoles

Milimoles of CO2 formed =   69.67 millimoles