Chapter 4Supplemental InstructionIowa State UniversityLeader: KatieCourse: Chem 177Instructor: KingstonDate: September 26, 20101. Define the following terms:a) saturated solution: b) unsaturated solution: c) supersaturated solution:d) concentration:e) molarity (equation): 2. a) Calculate the molarity of a solution that contains 0.0250 mol NH4Cl in exactly 500 mL of solution. b) How many moles of HNO3 are present in 50.0 mL of a 2.50M solution of nitric acid?c) How many millimeters of 1.50M KOH solution are needed to provide 0.275 mol of KOH? 3. a) You have a stock solution of 14.8M NH3 . How many milliliters of this solution shouldyou dilute to make 1000.0mL of 0.250M NH3 ? b) If you take a 10.0-mL portion of the stock solution and dilute it to a total volume of 0.500L, what will be the concentration of the final solution?Supplemental Instruction1060 Hixson-Lied Student Success Center v 294-6624 v www.si.iastate.edu4. Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodim bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid as follows:2NaHCO3(s) + H2SO4(aq) Na2SO4(aq) + 2H2O(l) + 2CO2(g) Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 27mL of 6.0M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the
View Full Document
Unlocking...