A student is given a 2.00-g mixture of sodium bicarbonate, anhydrous citric acid and corn starch. The student places all 2.00 g of the mixture in a gel capsule inside an Erlenmeyer flask and sets up a gas collection apparatus like below. She then adds 10.0 mL of 2.0 M HCI to the flask and quickly places the rubber stopper over the flask. Once the reaction is complete, the student collects 6.0 x 10-3 moles of dry carbon dioxide gas. She then titrates the leftover solution with 1.0 M NaOH and phenolphthalein as the indicator. The initial volume reading from the buret is 0.00 mL. The solution reaches its endpoint at 17.35 mL. A. Write the balance chemical reaction for citric acid and sodium bicarbonate
B. Write the balance to Chemical reaction for hydrochloric acid and sodium bicarbonate
C. What was the mass of each component in the original 2.00 g mixture show all work
D. In another sample of the same mixture after adding 10 mL of 2.0 M HCl a student from the sodium bicarbonate to be approximately .45 g of the 3.00 g solution when the remaining make sure it was titrated it took 23.40 mL of the 1.0 M NaOH to reach the endpoint what was the amount of citric acid in the ex show all work