Small quantities of hydrogen gas can be prepared in the laboratory by placing zinc metal in aqueous hydrochloric acid. Typically the hydrogen gas is bubbled through water for ease of collection and it becomes saturated with water vapor. Suppose 240. ml of hydrogen gas is collected over water at 30 degrees C and a barometric pressure of 1.032 atm. (The vapor pressure of water at 3 degrees is 32 torr) a. What is the minimum volume of a 50 % by mass solution of hydrochloric acid required to react with all of the zinc? Assume the density of the hydrochloric acid solution is 1.00 g/ml. b. To ensure all the zinc reacts, 25 % more hydrochloric acid is used than the minimum required. What is the concentration of the ions in solution after the reaction is complete?