1. Forgetful Freddy weighed his KHP sample, but forgot to bring his report sheet along, so he recorded the mass of KHP on a paper towel. During his titration, which required18.46 mL of base, he spilled some base on his hands. He remembered to wash his hands, but forgot about the data on the towel, and used it to dry his hands. When he went to        calculate the molarity of his base, Freddy discovered that he didn’t have the mass of his KHP. His kindhearted instructor told Freddy that his base was 0.2987 M. Calculate the mass of Freddy’s KHP sample. 2. What mass of solid NaOH would be needed to make 645 mL of Freddy’s NaOH solution?

5. A student conducted a titration experiment. He/she used 12.0 mL of silver nitrate (titrant) solution to reach the endpoint. If the student used 25.4 mL of the chloride (analyte) for the titration and found the concentration of chloride ions to be 2.2 M, what is the mass (in grams) of silver nitrate titrant Clic)

A student is given 1.52 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.650 M NaOH. The equivalence point is reached when 52.0 mL are added. Answer the following questions to determine the identity of the unknown acid. 1. How many moles of NaOH are consumed? Moles of NaOH = _____ mol 2. How many moles of H+ acid are available to react if the acid is H2C2O4? 0.0403 mol NaOH Moles of H+ from H2C2O4 = ___ mol 3. How many moles of H+ are available to react if the acid is H3C6H5O7? 0.0403 mol NaOH 0.0573 mol H+ from H2C2O4 Moles of H+ from H3C6H5O7 =  ___ mol

3. A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 3% H₂O₂. Reaction: SO2(g) + H₂O2 → H₂SO4. A 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H₂SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCI. Calculate the sulfur concentration in the sample in parts per million.