If it required 23.9 mL of 0.0150 M Ca(OH)2 to neutralize 25.0 mL of HNO3 , what was the initial concentration of the nitric acid solution?

A chemist needs to determine the concentration of a solution of nitric acid, HNO3 . She puts 905 mL of the acid in a flask along with a few drops of indicator. She then slowly adds 0.600 mol L-1 Ba(OH)2 to the flask until the solution turns pink, indicating the equivalence point of the titration. She notes that 275 mL of Ba(OH)2 equivalence point. was needed to reach the Solution map In this titration, the concentration of base is known and can be used to calculate the unknown acid concentration: concentration of base → moles of base → moles of acid → concentration of acid Part A How many moles of Ba(OH)2 are present in 275 mL of 0.600 mol L-1 Ba(OH)2 ? Express your answer numerically in moles. • View Available Hint(s) 0.165 mol Ba(OH)2 Submit Previous Answers v Correct Part B How many moles of HNO3 are present if 0.165 mol of Ba(OH)2 was needed to neutralize the acid solution? Express your answer numerically in moles. • View Available Hint(s) I* (3 E3 ? mol HNO3

Ag+(aq) + Cl-(aq) —> AgCl(s) What volume un milliliter a of 8.75 x 10^-2M sodium chloride solution (Nacl) would be required to completely precipitate the Ag+ ion from one liter of waste water that is 9.00 x 10^-4M in Ag+ ion?